20:11Stoichiometry - Limiting & Excess Reactant, Theoretical & Percent Yield - ChemistryThe Organic Chemistry Tutor435views1rank
25:16Stoichiometry Basic Introduction, Mole to Mole, Grams to Grams, Mole Ratio Practice ProblemsThe Organic Chemistry Tutor767views
Multiple ChoiceAmmonium nitrate (NH4NO3), a common fertilizer, is 35.0% nitrogen by mass. How much ammonium nitrate contains 1.25 kg of nitrogen?430views
Multiple ChoiceZeatin, a plant hormone, is known to have 5 nitrogen atoms in every molecule. Nitrogen makes up 33.8% of the mass of the molecule. What is the mass of one molecule in amu?194views
Multiple ChoiceIf a match contained 1.00 g of P, how much P4O10 would form if the following equation was obeyed? ___ KClO3 + ___ P → 10 KCl + ___ P4O10195views
Multiple ChoiceIn order to calculate the mass of a product in a chemical reaction from the number of moles of a reactant, which of the following describes all the conversion factors needed?1118views
Multiple ChoiceIn the following equation how many moles of aluminum chloride are produced from 2.50 mol of hydrochloric acid? 2 Al (s) + 6 HCl(aq) → 2 AlCl3 (aq) + 3 H2 (g)356views1rank
Multiple ChoiceWhen heated, potassium chlorate decomposes to potassium chloride and molecular oxygen: 2 KClO3 → 2 KCl + 3 O2 How much oxygen could be formed from 5.0 g of potassium chlorate?980views
Multiple ChoiceThe combination reaction for the formation of hydrazine is shown below:4 NH3 (g) + N2 (g) → 3 N2H4 (l)Determine the number of moles of hydrazine formed when 25.7 g ammonia reacts with excess nitrogen gas.159viewsHas a video solution.
Multiple ChoiceThe reaction between solid phosphorus and fluorine is given below:P4 (s) + 12 F2 (g) → 4 PF6 (aq)If 6.92 x 10-5 molecules of solid phosphorus react to completion, how many grams of phosphorus hexafluoride would be produced?157views1rank2commentsHas a video solution.
Multiple ChoiceDetermine the density of 50.0 mL iron (II) bromide when the following chemical reaction produced 112.7 g iron (II) phosphate.2 K3PO4 (aq) + 3 FeBr2 (aq) → Fe3(PO4)2 (s) + 6 KBr (aq)146views1rankHas a video solution.
Textbook QuestionOne way to make coal burning better for the environment is to remove carbon dioxide from the exhaust gases released from power plants using a compound containing an amine (-NH2) group. The reaction between carbon dioxide and monoethanolamine is: CO2(g) + 2 HOCH2CH2NH2(aq) -> HOCH2CH2NH3 +(aq) + HOCH2CH2NHCO2-(aq) What mass of monoethanoloamine is required to react with 1.0 kg of carbon dioxide? (LO 3.5) (a) 2.8 kg (b) 1.1 kg (c) 0.93 kg (d) 0.53 kg592viewsHas a video solution.
Textbook QuestionThe following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4. Based on this reaction, how many moles of H2 can be obtained starting with 4.0 mol CH4?336viewsHas a video solution.
Textbook QuestionThe following diagram represents a high-temperature reaction between CH4 and H2O. Based on this reaction, find how many moles of each product can be obtained starting with 4.0 mol CH4. Based on this reaction, find how many moles of CO can be obtained starting with 4.0 mol CH4?670views1rankHas a video solution.
Textbook QuestionConsider the unbalanced equation for the neutralization of acetic acid: HC2H3O2(aq) + Ba(OH)2(aq)¡H2O(l ) + Ba(C2H3O2)2(aq) Balance the equation and determine how many moles of Ba(OH)2 are required to completely neutralize 0.461 mole of HC2H3O2.1830viewsHas a video solution.
Textbook QuestionCalculate how many moles of NO2 form when each quantity of reactant completely reacts. 2 N2O5( g)¡4 NO2( g) + O2( g) a. 2.5 mol N2O55867viewsHas a video solution.
Textbook QuestionCalculate how many moles of NH3 form when each quantity of reactant completely reacts. 3 N2H4(l )¡4 NH3( g) + N2( g) c. 65.3 g N2H41541viewsHas a video solution.
Textbook QuestionConsider the balanced equation: SiO2(s) + 3 C(s)¡SiC(s) + 2 CO(g) Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms. Mol siO2 Mol C Mol SiC Mol CO _____ 1.55 _____ _____1009viewsHas a video solution.
Textbook QuestionConsider the balanced equation: SiO2(s) + 3 C(s)¡SiC(s) + 2 CO(g) Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product that forms. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that forms. Mol siO2 Mol C Mol SiC Mol CO _____ _____ _____ 10932viewsHas a video solution.
Textbook QuestionHydrobromic acid dissolves solid iron according to the reaction: Fe(s) + 2 HBr(aq)¡FeBr2(aq) + H2( g) What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?421viewsHas a video solution.
Textbook QuestionHydrobromic acid dissolves solid iron according to the reaction: Fe(s) + 2 HBr(aq)¡FeBr2(aq) + H2( g) What mass of HBr (in g) do you need to dissolve a 3.2-g pure iron bar on a padlock?3651viewsHas a video solution.
Textbook QuestionSulfuric acid dissolves aluminum metal according to the reaction: 2 Al(s) + 3 H2SO4(aq)¡Al2(SO4)3(aq) + 3 H2( g) Suppose you want to dissolve an aluminum block with a mass of 15.2 g. What minimum mass of H2SO4 (in g) do you need? What mass of H2 gas (in g) does the complete reaction of the aluminum block produce?10615views4rank1commentsHas a video solution.
Textbook QuestionCytosine, a constituent of deoxyribonucleic acid (DNA), can be represented by the following molecular model. If 0.001 mol of cytosine is submitted to combustion analysis, how many moles of CO2 and how many moles of H2O would be formed? (Gray = C, red = O, blue = N, ivory = H.)515views1rankHas a video solution.
Textbook QuestionFor each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant. d. 2 Sr(s) + O2( g)¡2 SrO(s)3190viewsHas a video solution.
Textbook QuestionFor each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO3(aq) + Ca(OH)2(aq)¡2 H2O(l ) + Ca(NO3)2(aq)864viewsHas a video solution.
Textbook QuestionThe organic anion is found in most detergents. Assume that the anion under-goes aerobic decomposition in the following manner: C18H29SO3- + 51 O2 → 36 CO2(aq) + 28 H2O (l) + 2 H+(aq) + 2 SO42-(aq) What is the total mass of O2 required to biodegrade 10.0 g of this substance?348viewsHas a video solution.
Textbook QuestionHydrofluoric acid, HF(aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF(aq). Sodium silicate 1Na2SiO32, for example, reacts as follows: Na2SiO31s2 + 8 HF1aq2¡ H2SiF61aq2 + 2 NaF1aq2 + 3 H2O1l2 (b) How many grams of NaF form when 0.500 mol of HF reacts with excess Na2SiO3?4982viewsHas a video solution.
Textbook QuestionIn the preparation of iron from hematite, Fe2O3 reacts with carbon: Fe2O3 + C --> Fe + CO2 Unbalanced (a) Balance the equation. (b) How many moles of carbon are needed to react with 525 g of hematite? (c) How many grams of carbon are needed to react with 525 g of hematite?1470viewsHas a video solution.
Textbook QuestionThe reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (b) How many grams of KO2 are needed to form 7.50 g of O2?589viewsHas a video solution.
Textbook QuestionThe reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (a) How many moles of O2 are produced when 0.400 mol of KO2 reacts in this fashion?1673viewsHas a video solution.
Textbook QuestionSeveral brands of antacids use Al1OH23 to react with stomach acid, which contains primarily HCl: Al1OH231s2 + HCl1aq2¡AlCl31aq2 + H2O1l2 (b) Calculate the number of grams of HCl that can react with 0.500 g of Al1OH23.557viewsHas a video solution.
Textbook QuestionMagnesium metal burns in oxygen to form magnesium oxide, MgO. (c) How many grams of Mg are needed to react with 25.0 g of O2? How many grams of MgO will result?672viewsHas a video solution.
Textbook QuestionMagnesium metal burns in oxygen to form magnesium oxide, MgO. (b) How many grams of oxygen are needed to react with 25.0 g of Mg? How many grams of MgO will result?1601viewsHas a video solution.
Textbook QuestionAn iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: Fe2O31s2 + CO1g2¡Fe1s2 + CO21g2 (b) Calculate the number of grams of CO that can react with 0.350 kg of Fe2O3.1202viewsHas a video solution.
Textbook QuestionEthylene gas, C2H4, reacts with water at high temperature to yield ethyl alcohol, C2H6O. (a) How many grams of ethylene are needed to react with 0.133 mol of H2O? How many grams of ethyl alcohol will result? (b) How many grams of water are needed to react with 0.371 mol of ethylene? How many grams of ethyl alcohol will result?2444viewsHas a video solution.
Textbook QuestionAluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from 14.2 g of aluminum sulfide?2288viewsHas a video solution.
Textbook QuestionPure oxygen was first made by heating mercury(II) oxide: HgO --> (heat) Hg + O2 Unbalanced (a) Balance the equation. (b) How many grams of mercury and how many grams of oxygen are formed from 45.5 g of HgO? (c) How many grams of HgO would you need to obtain 33.3 g of O2709viewsHas a video solution.
Textbook QuestionTitanium dioxide (TiO2), the substance used as the pigment in white paint, is prepared industrially by reaction of TiCl4 with O2 at high temperature. TiCl4 + O2 --> (heat) TiO2 + 2 Cl2 How many kilograms of TiO2 can be prepared from 5.60 kg of TiCl4?1614viewsHas a video solution.
Textbook QuestionAutomotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2 NaN31s2¡2 Na1s2 + 3 N21g2 (c) How many grams of NaN3 are required to produce 10.0 ft3 of nitrogen gas, about the size of an automotive air bag, if the gas has a density of 1.25 g/L?659viewsHas a video solution.
Textbook QuestionAutomotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements: 2 NaN31s2¡2 Na1s2 + 3 N21g2 (c) How many grams of NaN3 are required to produce 10.0 ft3 of nitrogen gas, about the size of an automotive air bag, if the gas has a density of 1.25 g/L?1931viewsHas a video solution.
Textbook QuestionThe complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H18 (l) + 25 O2 (g) → 16 CO2 (g) + 18 H2O (g) (c) Octane has a density of 0.692 g/mL at 20 °C. How many grams of O2 are required to burn 15.0 gal of C8H18 (the capacity of an average fuel tank)?16166viewsHas a video solution.
Textbook QuestionThe complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H181l2 + 25 O21g2¡16 CO21g2 + 18 H2O1g2 (a) How many moles of O2 are needed to burn 1.50 mol of C8H18?1146viewsHas a video solution.
Textbook QuestionThe complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2 C8H181l2 + 25 O21g2¡16 CO21g2 + 18 H2O1g2 (b) How many grams of O2 are needed to burn 10.0 g of C8H18?1245viewsHas a video solution.
Textbook QuestionThe industrial production of hydriodic acid takes place by treatment of iodine with hydrazine (N2H4): 2 I2 + N2H4 --> 4 HI + N2 (b) How many grams of HI are produced from the reaction of 115.7 g of N2H4 with excess iodine661viewsHas a video solution.
Textbook QuestionDetonation of nitroglycerin proceeds as follows: 4 C3H5N3O91l2¡ 12 CO21g2 + 6 N21g2 + O21g2 + 10 H2O1g2 (a) If a sample containing 2.00 mL of nitroglycerin 1density = 1.592 g>mL2 is detonated, how many moles of gas are produced?1035views1rankHas a video solution.
Textbook QuestionAn alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide: H2S + I2 --> 2 HI + S (b) How many grams of HI are produced from the reaction of 95.4 g of H2S with excess I2?416viewsHas a video solution.
Textbook QuestionAn alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide: H2S + I2 --> 2 HI + S (a) How many grams of I2 are needed to react with 49.2 g of H2S?454viewsHas a video solution.
Textbook QuestionNickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid: NiCO3 + H2SO4 --> NiSO4 + CO2 + H2O (a) How many grams of H2SO4 are needed to react with 14.5 g of NiCO3?940viewsHas a video solution.
Textbook QuestionHydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 --> N2 + 2 H2O (a) How many grams of O2 are needed to react with 50.0 g of N2H4?1156viewsHas a video solution.
Textbook QuestionDuring a period of discharge of a lead–acid battery, 402 g of Pb from the anode is converted into PbSO41s2. (a) What mass of PbO21s2 is reduced at the cathode during this same period?597viewsHas a video solution.
Textbook QuestionSodium azide (NaN3) yields N2 gas when heated to 300 °C, a reaction used in automobile air bags. If 1.00 mol of N2 has a volume of 47.0 L under the reaction conditions, how many liters of gas can be formed by heating 38.5 g of NaN3? The reaction is1319viewsHas a video solution.
Textbook QuestionThe reaction of tungsten hexachloride (WCl6) with bismuth gives hexatungsten dodecachloride (W6Cl12). WCl6 + Bi ---> W6Cl12 + BiCl3 Unbalanced (b) How many grams of bismuth react with 150.0 g of WCl6?499viewsHas a video solution.
Textbook QuestionIf 2.0 mol CH3CH2CH2COOH, 2.0 mol C4H10, and 2.0 mol C6H6 are completely combusted in oxygen, which one produces the largest number of moles of H2O?391viewsHas a video solution.
Textbook QuestionHow many kilograms of CO2 does the complete combustion of 3.8 kg of n-octane produce?890viewsHas a video solution.
Textbook QuestionAn element X forms an iodide 1XI32 and a chloride 1XCl32. The iodide is quantitatively converted to the chloride when it is heated in a stream of chlorine: 2 XI3 + 3 Cl2¡2 XCl3 + 3 I2 If 0.5000 g of XI3 is treated with chlorine, 0.2360 g of XCl3 is obtained. (a) Calculate the atomic weight of the element X.826viewsHas a video solution.
Textbook QuestionA method used by the U.S. Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the air sample through a 'bubbler' containing sodium iodide, which removes the ozone according to the following equation: O31g2 + 2 NaI1aq2 + H2O1l2¡ O21g2 + I21s2 + 2 NaOH1aq2 (a) How many moles of sodium iodide are needed to remove 5.95 * 10-6 mol of O3?365viewsHas a video solution.
Textbook QuestionA method used by the U.S. Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the air sample through a 'bubbler' containing sodium iodide, which removes the ozone according to the following equation: O31g2 + 2 NaI1aq2 + H2O1l2¡ O21g2 + I21s2 + 2 NaOH1aq2 (b) How many grams of sodium iodide are needed to remove 1.3 mg of O3?477viewsHas a video solution.
Textbook QuestionThe fat stored in a camel's hump is a source of both energy and water. Calculate the mass of H2O produced by the metabolism of 1.0 kg of fat, assuming the fat consists entirely of tristearin 1C57H110O62, a typical animal fat, and assuming that during metabolism, tristearin reacts with O2 to form only CO2 and H2O.1340viewsHas a video solution.
Textbook QuestionHard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. Keep in mind that charge balance must be maintained. (b) If the sodium is added to the water softener in the form of NaCl, how many grams of sodium chloride are needed?766viewsHas a video solution.
Textbook QuestionA mixture of N21g2 and H21g2 reacts in a closed container to form ammonia, NH31g2. The reaction ceases before either reactant has been totally consumed. At this stage 3.0 mol N2, 3.0 mol H2, and 3.0 mol NH3 are present. How many moles of N2 and H2 were present originally?825viewsHas a video solution.
Textbook QuestionA mixture containing KClO3, K2CO3, KHCO3, and KCl was heated, producing CO2, O2, and H2O gases according to the following equations: 2 KClO31s2¡2 KCl1s2 + 3 O21g2 2 KHCO31s2¡K2O1s2 + H2O1g2 + 2 CO21g2 K2CO31s2¡K2O1s2 + CO21g2 The KCl does not react under the conditions of the reaction. If 100.0 g of the mixture produces 1.80 g of H2O, 13.20 g of CO2, and 4.00 g of O2, what was the composition of the original mixture? (Assume complete decomposition of the mixture.) How many grams of K2CO3 were in the original mixture?1172viewsHas a video solution.
Textbook QuestionThe combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)7946viewsHas a video solution.
Textbook QuestionMany home barbeques are fueled with propane gas (C3H8). What mass of carbon dioxide (in kg) is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gallon tank)? Assume that the density of the liquid propane in the tank is 0.621 g>mL. (Hint: Begin by writing a balanced equation for the combustion reaction.)1402viewsHas a video solution.
Textbook QuestionAssume that gasoline has the formula C8H18 and has a density of 0.703 g/mL. How many pounds of CO2 are produced from the complete combustion of 1.00 gal of gasoline?3834viewsHas a video solution.
Textbook QuestionA 3.50 g of an alloy which contains only lead and tin is dissolved in hot HNO3. Excess sulfuric acid is added to this solution and 1.57g of PbSO4(s) is obtained. (b) Assuming all the lead in the alloy reacted to form PbSO4, what was the amount, in grams, of lead and tin in the alloy respectively?511viewsHas a video solution.
Textbook QuestionA certain alcoholic beverage contains only ethanol (C2H6O) and water. When a sample of this beverage undergoes com-bustion, the ethanol burns but the water simply evaporates and is collected along with the water produced by combus-tion. The combustion reaction is When a 10.00 g sample of this beverage is burned, 11.27 g of water is collected. What is the mass in grams of ethanol, and what is the mass of water in the original sample?593viewsHas a video solution.
Textbook QuestionThe source of oxygen that drives the internal combustion engine in an automobile is air. Air is a mixture of gases, principally N2179%2 and O2120%2. In the cylinder of an automobile engine, nitrogen can react with oxygen to produce nitric oxide gas, NO. As NO is emitted from the tailpipe of the car, it can react with more oxygen to produce nitrogen dioxide gas. (c) The production of NOx gases is an unwanted side reaction of the main engine combustion process that turns octane, C8H18, into CO2 and water. If 85% of the oxygen in an engine is used to combust octane and the remainder used to produce nitrogen dioxide, calculate how many grams of nitrogen dioxide would be produced during the combustion of 500 g of octane.1447viewsHas a video solution.
Textbook QuestionThe YBa2Cu3O7 superconductor can be synthesized by the sol–gel method from a stoichiometric mixture of metal ethoxides followed by heating in oxygen. How many grams of Y1OCH2CH323 and how many grams of Ba1OCH2CH322 are required to react with 75.4 g of Cu1OCH2CH322 and an excess of water? Assuming a 100% yield, how many grams of YBa2Cu3O7 are obtained?428viewsHas a video solution.
Textbook QuestionA compound of formula XCl3 reacts with aqueous AgNO3 to yield solid AgCl according to the following equation: When a solution containing 0.634 g of XCl3 was allowed to react with an excess of aqueous AgNO3, 1.68 g of solid AgCl was formed. What is the identity of the atom X?284viewsHas a video solution.
Textbook QuestionThe thermite reaction, Fe2O3 + Al S Al2O3 + Fe produces so much heat that the Fe product melts. This reaction is used industrially to weld metal parts under water, where a torch cannot be employed. It is also a favorite chemical demonstration in the lecture hall (on a small scale). (b) Calculate how many grams of aluminum are needed to completely react with 500.0 g of Fe2O3 in this reaction.5287viewsHas a video solution.
Textbook QuestionPotassium superoxide, KO2, is often used in oxygen masks (such as those used by firefighters) because KO2 reacts with CO2 to release molecular oxygen. Experiments indicate that 2 mol of KO21s2 react with each mole of CO21g2. (c) What mass of KO21s2 is needed to consume 18.0 g CO21g2? What mass of O21g2 is produced during this reaction?1481viewsHas a video solution.
Textbook QuestionWhen eaten, dietary carbohydrates are digested to yield glu-cose (C6H12O6), which is then metabolized to yield carbon dioxide and water: Balance the equation, and calculate both the mass in grams and the volume in liters of the CO2 produced from 66.3 g of glucose, assuming that 1 mol of CO2 has a volume of 25.4 L at normal body temperature.458viewsHas a video solution.
Textbook QuestionWindow glass is typically made by mixing soda ash (Na2CO3), limestone (CaCO3), and silica sand (SiO2) and then heating to 1500 °C to drive off CO2 from the (Na2CO3) and CaCO3. The resultant glass consists of about 12% Na2O by mass, 13% CaO by mass, and 75% SiO2 by mass. How much of each reactant would you start with to prepare 0.35 kg of glass?1416viewsHas a video solution.
Textbook QuestionAn unidentified metal M reacts with an unidentified halogen X to form a compound MX2. When heated, the compound decomposes by the reaction: When 1.12 g of MX2 is heated, 0.720 g of MX is obtained, along with 56.0 mL of X2 gas. Under the conditions used, 1.00 mol of the gas has a volume of 22.41 L. (a) What is the atomic weight and identity of the halogen X?420viewsHas a video solution.
Textbook QuestionThe reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated. Find the mass of PH3 that forms from the reaction of 1.00 g of NH3.2084viewsHas a video solution.
Textbook QuestionAn important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO2 from Fe2O3 and CO. Determine the mass of Fe2O3 required to form 910 kg of iron. Determine the amount of CO2 that forms in this process.2521views2rankHas a video solution.
Textbook QuestionA liquid fuel mixture contains 30.35% hexane (C6H14), 15.85% heptane (C7H16), and the rest octane (C8H18). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?2975viewsHas a video solution.
Textbook QuestionOne method to synthesize ionic solids is by the heating of two reactants at high temperatures. Consider the reaction of FeO with TiO2 to form FeTiO3. Determine the amount of each of the two reactants to prepare 2.500 g FeTiO3, assuming the reaction goes to completion. (d) Determine moles and mass (g) of FeO required.409viewsHas a video solution.
Textbook QuestionA mixture of CuO and Cu2O with a mass of 10.50 g is reduced to give 8.66 g of pure Cu metal. What are the amounts in grams of CuO and Cu2O in the original mixture?877viewsHas a video solution.
Textbook QuestionWhen the nickel–zinc battery, used in digital cameras, is recharged, the following cell reaction occurs: (a) How many grams of zinc are formed when 3.35 x 10^-2 g of Ni(OH)2 are consumed?239viewsHas a video solution.
Textbook QuestionIsooctane, C8H18, is the component of gasoline from which the term octane rating derives. (b) Assuming that gasoline is 100% isooctane, that isooctane burns to produce only CO2 and H2O, and that the density of isooctane is 0.792 g/mL, what mass of CO2 in kilograms is produced each year by the annual U.S. gasoline consumption of 4.6 * 1010 L?1049viewsHas a video solution.
Textbook QuestionAcid spills are often neutralized with sodium carbonate or sodium hydrogen carbonate. For neutralization of acetic acid, the unbalanced equations are 112 CH3CO2H1l2 + Na2CO31s2 S CH3CO2Na1aq2 + CO21g2 + H2O1l2 122 CH3CO2H1l2 + NaHCO31s2 CH3CO2Na1aq2 + CO21g2 + H2O1l2 (b) How many kilograms of each substance is needed to neu- tralize a 1.000-gallon spill of pure acetic acid 1density = 1.049 g>mL2?1367viewsHas a video solution.
Textbook QuestionA railroad tank car derails and spills 36 tons of concen-trated sulfuric acid. The acid is 98.0 mass% H2SO4 and has a density of 1.836 g/mL. (b) How many kilograms of sodium carbonate are needed to completely neutralize the acid?380viewsHas a video solution.
Textbook QuestionSome progressive hair coloring products marketed to men, such as Grecian Formula 16, contain lead acetate Pb(CH3CO2)2. As the coloring solution is rubbed on the hhair, the Pb2+ ions react with the sulfur atoms in hair proteins to give lead(II) sulfide (PbS), which is black. A typical coloring solution contains 0.3 mass% Pb(CH3CO2)2, and about 2 mL of the solution is used per application. (a) Assuming that 30% of the Pb(CH3CO2)2 is converted to PbS, how many milligrams of PbS are formed per application of the coloring solution?478viewsHas a video solution.
Textbook QuestionDuring a certain time period, 4.0 million tons of SO2 were released into the atmosphere and subsequently oxidized to SO3. As explained in the Inquiry, the acid rain produced when the SO3 dissolves in water can damage marble statues: CaCO31s2 + H2SO41aq2S CaSO41aq2 + CO21g2 + H2O1l2 (a) How many 500 pound marble statues could be damaged by the acid rain? (Assume that the statues are pure CaCO3 and that a statue is damaged when 3.0% of its mass is dissolved.)310viewsHas a video solution.
Open QuestionHow many moles of nitrogen are needed to completely convert 6.34 mol of hydrogen?159viewsHas a video solution.
Open QuestionHow many chlorine atoms are on the products side of the reaction 2Al + 6HCl ‚Üí 2AlCl3 + 3H2? 2 3 6 9170viewsHas a video solution.
Open QuestionHow many moles of hexane (C6H14) must burn to form 18.4 mol of carbon dioxide?132viewsHas a video solution.
Open QuestionConsider the balanced equation below. What is the mole ratio of Fe?130viewsHas a video solution.
Open QuestionExplain the concept of mole ratio as used in reaction stoichiometry problems134viewsHas a video solution.
Open QuestionCalculate the amount of Al2O3 if 351 grams of al is reacted with excess O2139viewsHas a video solution.
Open QuestionWhat mass of silver oxide, Ag2O, is required to produce 25.0 g of silver sulfadiazine, AgC10H9N4SO2, from the reaction of silver oxide and sulfadiazine?153viewsHas a video solution.
Open QuestionWhat mass of h2 would be produced by the complete reaction of the iron bar?261viewsHas a video solution.
Open QuestionThe coefficients in a balanced chemical equation always can express the ratio of243viewsHas a video solution.
Open QuestionBased on the mole ratios, what can most likely be predicted?208viewsHas a video solution.
Open QuestionHow many moles of oxygen are produced if 11.0 mol of Al are produced?177viewsHas a video solution.
Open QuestionAmmonia NH3 chemically reacts with oxygen gas O2 to produce nitric oxide NO and water H2O.123viewsHas a video solution.
Open QuestionGiven 6.000 moles of aluminum (Al), how many grams of aluminum oxide (Al2O3) will be produced?109viewsHas a video solution.
Open QuestionThe molar mass of O2 is 32.0 g/mol. What mass, in grams, of O2 must react to form 3.80 mol of Al2O3?258viewsHas a video solution.
Open QuestionHow many moles of copper must react to form 3.50 mol of Ag? 0.175 mol 1.75 mol 7.00 mol 17.0 mol114viewsHas a video solution.
Open QuestionCalculate the number of grams of oxygen required to convert 63.0 g of glucose to CO2 and H2O.132viewsHas a video solution.
Open QuestionHow many grams of oxygen gas are needed to produce 36.0 grams of water?103viewsHas a video solution.
Open QuestionThe number of moles of hydrogen that is needed to produce 0.253 mol of water is110viewsHas a video solution.
Open QuestionWhat are the mole ratios of hydrazine (N2H4) to hydrogen peroxide (H2O2) and hydrazine to water?88viewsHas a video solution.
Open QuestionHow many moles of oxygen (O2) are required to react completely with 1.67 mol H2?155views
Open QuestionHow many moles of CO2 are produced when 5.80 mol of ethane are burned in an excess of oxygen?160viewsHas a video solution.
Open QuestionConsider the balanced equation below. What is the mole ratio of PCl3 to PCl5?103viewsHas a video solution.
Open QuestionWhat mass of NaCl can be produced by the reaction of 5.0 mol Cl2? 2 Na + Cl2 --> 2 NaCl98viewsHas a video solution.
Open QuestionIf you produced 5 moles of Ca3(PO4)2, how many moles of NaCl did you also produce?103viewsHas a video solution.