05:11STP Gas Chemistry (Standard Temperature and Pressure) Examples Practice Problems Questions ShortcutConquer Chemistry964views
Multiple ChoiceA sample of dichloromethane gas (CH2Cl2) occupies 32.6 L at 310 K and 5.30 atm. Determine its volume at STP?699views2rank1comments
Multiple ChoiceNitrogen and hydrogen combine to form ammonia via the following reaction: 1 N2 (s) + 3 H2 (g) → 2 NH3 (g)What mass of nitrogen is required to completely react with 800.0 mL H2 at STP?18485views2comments
Multiple ChoiceWhat is the pressure inside a 1.5-L container that is charged with 3.0 moles of a gas at 35.0℃?367views1rank
Multiple ChoiceThe combustion of glucose yields carbon dioxide and water according to the following reaction: C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) Calculate the mass of H2O produced when 12.0 g of glucose is combusted in a container of oxygen with a volume of 1.3 L at a pressure of 2.2 atm and a temperature of 205℃.4250views
Textbook QuestionPropane gas 1C3H82 is often used as fuel in rural areas. How many liters of CO2 are formed at STP by the complete combustion of the propane in a container with a volume of 15.0 L and a pressure of 4.50 atm at 25.0 °C? The equation for the combustion of propane is: C3H81g2 + 5 O21g2¡3 CO21g2 + 4 H2O1l2 (LO 10.4, 10.5) (a) 61.8 L (b) 186 L (c) 20.6 L (d) 2.21 * 103 L516views
Textbook QuestionAt standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (b) On cooling to 160 K, both substances form crystalline solids. Do you expect the molar volumes to decrease or increase on cooling the gases to 160 K?604views
Textbook QuestionAt standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (c) The densities of crystalline Cl2 and NH3 at 160 K are 2.02 and 0.84 g/cm3, respectively. Calculate their molar volumes.2407views
Textbook QuestionChlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 119.3 kPa and 24 °C. (b) What volume will the Cl2 occupy at STP?1084views
Textbook QuestionMany gases are shipped in high-pressure containers. Consider a steel tank whose volume is 210.0 L that contains O2 gas at a pressure of 16,500 kPa at 23 °C. (b) What volume would the gas occupy at STP?602views
Textbook QuestionThe surface temperature of Venus is about 1050 K, and the pressure is about 75 Earth atmospheres. Assuming that these conditions represent a Venusian 'STP,' what is the standard molar volume in liters of a gas on Venus?988views
Textbook QuestionWhich sample contains more molecules: 1.00 L of O2 at STP, 1.00 L of air at STP, or 1.00 L of H2 at STP?980views
Textbook QuestionA compressed air tank carried by scuba divers has a volume of 8.0 L and a pressure of 140 atm at 20 °C. What is the volume of air in the tank in liters at STP?1675views
Textbook QuestionUse the molar volume of a gas at STP to determine the volume (in L) occupied by 33.6 g of neon at STP.1921views
Textbook QuestionUse the molar volume of a gas at STP to calculate the density (in g>L) of nitrogen gas at STP.2997views1rank
Textbook QuestionImagine that you have two identical flasks, one containing hydrogen at STP and the other containing oxygen at STP. How can you tell which is which without opening them?458views
Textbook QuestionOne mole of an ideal gas has a volume of 22.414 L at STP. Assuming ideal behavior, what are the densities of the following gases in g/L at STP? (a) CH4 (b) CO2 (c) O23055views
Textbook QuestionWhat are the molecular weights of the gases with the following densities: (a) 1.342 g/L at STP468views
Textbook QuestionTitanium(III) chloride, a substance used in catalysts for preparing polyethylene, is made by high-temperature reaction of TiCl4 vapor with H2: 2 TiCl41g2 + H21g2¡2 TiCl31s2 + 2 HCl1g2 (b) How many liters of HCl gas at STP will result from the reaction described in part (a)?383views
Textbook QuestionAutomobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 2 NaN3(s)¡2 Na(s) + 3 N2( g) If an automobile air bag has a volume of 11.8 L, what mass of NaN3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions.6089views1rank3comments
Textbook QuestionLithium reacts with nitrogen gas according to the reaction: 6 Li(s) + N2( g)¡2 Li3N(s) What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?1726views
Textbook QuestionHydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: CH4( g) + H2O( g)¡CO( g) + 3 H2( g) In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?5155views
Textbook QuestionSuppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (b) density?393views
Textbook QuestionSuppose you have two 1-L flasks, one containing N2 at STP, the other containing CH4 at STP. How do these systems compare with respect to (a) number of molecules?453views
Textbook QuestionA gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, was 0.646 g. What is the molecular formula of the compound?2568views3rank
Textbook QuestionConsider the reaction: 2 SO2( g) + O2( g)¡2 SO3( g) a. If 285.5 mL of SO2 reacts with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and the theoretical yield of SO3?1295views
Textbook QuestionThe Earth's atmosphere has a mass of approximately 5.15 * 1015 kg. If the average molar mass of air is 28.8 g/mol, how many moles of gas make up the atmosphere? What is the volume of the atmosphere in liters under conditions of STP? (Note: The average molar mass of air is the weighted average of the molar mass of nitrogen and oxygen. 0.20132.0 g>mol2 + 0.80128.0 g>mol2 = 28.8 g>mol.)1424views
Textbook QuestionAn herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor expressed at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. (b) Calculate its empirical formula.1705views
Textbook QuestionIsooctane, C8H18, is the component of gasoline from which the term octane rating derives. (d) How many moles of air are necessary for the combustion of 1 mol of isooctane, assuming that air is 21.0% O2 by volume? What is the volume in liters of this air at STP?683views
Open QuestionApproximately how many moles of Kr+ are contained in the laser tube at 0°C and 1 atm?285views
Open QuestionUse the molar volume of a gas at STP to calculate the density (in g/l) of nitrogen gas at STP.173views
Open QuestionWhat is the volume of 3.5 moles of oxygen gas (O2) at standard temperature and pressure (STP)?189views
Open QuestionWhich gas occupies the highest volume at STP? 0.02 mol of O20.1 mol of Cl21 mol of N22 mol of H2146views
Open Question2.00 g of an unknown gas at stp fills a 500 mL flask. What is the molar mass of the gas?238views
Open QuestionWhat is the mass of 3.45l of gaseous ammonia (NH3) at STP? Round to 3 significant figures.146views
Open QuestionWhat is the volume of 1.2 moles of oxygen gas (O2) at standard temperature and pressure (STP)?146views