02:56Reactivity Series of Metals | Environmental | Chemistry | FuseSchoolFuseSchool - Global Education903views
04:08Making Predictions Using Reactivity Series | Reactions | Chemistry | FuseSchoolFuseSchool - Global Education431views
Multiple ChoiceBased on your understanding of activities determine if a reaction occurs and if so provide the products formed. Ba (s) + H2O (g) →281views1rank1comments
Multiple ChoiceBased on your understanding of activities determine if a reaction occurs and if so provide the products formed. Zn (s) + NiCl2 (aq) →262views2rank
Multiple ChoiceIf the activity of halogens is stated as:Fluorine > Chlorine > Bromine > Iodine, determine if a reaction occurs and if so provide the products formed. Cl2 (g) + AlBr3 (aq) →307views5rank1comments
Textbook QuestionThe most strongly reducing elements are listed at the top of the partial activity series table provided. Use the activity series to predict which reaction will occur. (LO 4.20) (a) (b) (c) (d) 261views
Textbook QuestionBased on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red+ + Green ---> Red + Green+ (b) Blue + Green+ ---> Blue+ + Green (c) Red + Blue+ ---> Red+ + Blue 387views
Textbook QuestionThe following two redox reactions occur between aqueous cations and solid metals. Will a solution of green cations react with solid blue metal? Explain. (a) (b) (c) (d) 343views
Textbook QuestionWrite balanced molecular and net ionic equations for the reactions of (d) aluminum with formic acid, HCOOH.730views
Textbook QuestionWrite balanced molecular and net ionic equations for the reactions of (d) acetic acid, CH3COOH, with zinc.460views
Textbook QuestionWrite balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron305views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) zinc metal is added to a solution of magnesium sulfate735views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) aluminum metal is added to a solution of cobalt(II) sulfate.410views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride739views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal531views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) hydrogen gas is bubbled through a solution of silver nitrate.571views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride722views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate594views
Textbook QuestionUsing the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate731views
Textbook QuestionThe metal cadmium tends to form Cd2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)(aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?899views
Textbook QuestionThe following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: Br21aq2 + 2 NaI1aq2¡2 NaBr1aq2 + I21aq2 Cl21aq2 + 2 NaBr1aq2¡2 NaCl1aq2 + Br21aq2 (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?621views
Textbook QuestionWrite the balanced chemical equation for the reaction of solid strontium with iodine gas.952views
Textbook QuestionWrite the balanced chemical equation for the reaction of solid lithium with liquid water.826views
Textbook QuestionWrite the balanced chemical equation for the reaction of solid potassium with liquid water.620views
Textbook QuestionWrite the balanced equation for the reaction of hydrogen gas with bromine gas.779views
Textbook QuestionAssume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?371views
Textbook QuestionConsider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution. (a) Given a 500-mL Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon?357views
Textbook QuestionBronze is a solid solution of Cu(s) and Sn(s); solutions of metals like this that are solids are called alloys. There is a range of compositions over which the solution is considered a bronze. Bronzes are stronger and harder than either copper or tin alone. (c) Suggest a reaction that you could do to remove all the tin from this bronze to leave a pure copper sample. Justify your reasoning.917views
Textbook QuestionSuppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (d) What is the molarity of Cu2+ ions in the resulting solution?345views
Textbook QuestionSuppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (a) Which metal will react with the copper(II) nitrate solution?322views
Textbook QuestionDetermine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. c. 2.42gAg368views
Textbook QuestionDetermine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. b. 4.85gCu471views
Textbook QuestionDetermine whether HI can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HI and determine the minimum volume of 3.5 M HI required to completely dissolve the sample. a. 2.15gAl697views
Textbook QuestionDetermine if HNO3 can dissolve each metal sample. If it can, write a balanced chemical reaction showing how the metal dissolves in HNO3 and determine the minimum volume of 6.0 M HNO3 required to completely dissolve the sample. a. 5.90gAu742views
Textbook QuestionUse the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (d)481views
Textbook QuestionUse the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (c)328views
Textbook QuestionUse the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (b)402views
Textbook QuestionUse the activity series of metals (Table 4.5) to predict the outcome of each of the following reactions. If no reaction occurs, write NR. (a)411views
Textbook Question(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?308views
Textbook Question(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:301views
Textbook Question(a) Use the following reactions to arrange the elements A, B, C, and D in order of their decreasing ability as reducing agents:411views
Textbook Question(b) Which of the following reactions would you expect to occur according to the activity series you established in part (a)?310views
Textbook QuestionChlorine dioxide gas 1ClO22 is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the ClO2 is itself reduced. (b) Why do you think that ClO2 is reduced so readily?546views
Textbook QuestionSome metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by (c) heating its oxide with coke?282views
Textbook QuestionSome metals occur naturally in their elemental state while others occur as compounds in ores. Gold, for instance, is found as the free metal; mercury is obtained by heating mercury(II) sulfide ore in oxygen; and zinc is obtained by heating zinc(II) oxide ore with coke (carbon). Judging from their positions in the activity series, which of the metals sil-ver, platinum, and chromium would probably be obtained by (a) finding it in its elemental state?1321views
Textbook QuestionA sample of metal (M) reacted with both steam and aqueous HCl to release H2 but did not react with water at room tem-perature. When 1.000 g of the metal was burned in oxygen, it formed 1.890 g of a metal oxide, M2O3. What is the iden-tity of the metal?587views
Textbook QuestionAn unknown metal (M) was found not to react with either water or steam, but its reactivity with aqueous acid was not investigated. When a 1.000 g sample of the metal was burned in oxygen and the resulting metal oxide converted to a metal sulfide, 1.504 g of sulfide was obtained. What is the identity of the metal?394views