Given the chemical equation below: Cl2 CI + CIO - What is the reducing agent? C12 What is the oxidizing agent? C12 How many electrons are lost and gained in the reaction? (positive integers only) 2 What is the lowest possible sum of the coefficients in the overall balanced equation? (assume all coefficients are positive integers)? 6

Given the chemical equation below: Cl2 CI + CIO - What is the reducing agent? C12 What is the oxidizing agent? C12 How many electrons are lost and gained in the reaction? (positive integers only) 2 What is the lowest possible sum of the coefficients in the overall balanced equation? (assume all coefficients are positive integers)? 6

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 7ALQ

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One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.
3.93 Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown be1ow.
The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?
4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
Write the balanced chemical equation for the complete combustion of adipic acid, an organic acid containing 49.31% C, 6.90% H, and the remainder O, by mass.
Although copper does not usually react with acids, it does react with concentrated nitric acid. The reaction is complicated, but one outcome is Cu(s)+HNO3(conc)Cu(NO3)2(aq)+NO2(g)+H2O(l) (a) Name all of the reactants and products. (b) Balance the reaction. (c) Assign oxidation numbers to the atoms. Is this a redox reaction? (d) Pre-1983 pennies were made of pure copper. If such a penny had a mass of 3.10 g, how many moles of Cu are in one penny? How many atoms of copper are in one penny? (e) What mass of HNO3 would be needed to completely react with a pre-1983 penny?
High cost and limited availability of a reactant often dictate which reactant is limiting in a particular process. Identify the limiting reactant when the reactions below are run, and come up with a reason to support your decision. a. Burning charcoal on a grill: C(s)+O2(g)CO2(g) b. Burning a chunk of Mg in water: Mg(s)+2H2O(l)Mg(OH)2(aq)+H2(g) c. The Haber process of ammonia production: 3H2(g)+N2(g)2NH3(g)
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
You are making cookies and are missing a key ingredient—eggs. You have plenty of the other ingredients, except that you have only 1.33 cups of butter and no eggs. You note that the recipe calls for 2 cups of butter and 3 eggs (plus the other ingredients) to make 6 dozen cookies. You telephone a friend and have him bring you some eggs. How many eggs do you need? If you use all the butter (and get enough eggs), how many cookies can you make? fortunately, your mend hangs up before you tell him how mans eggs you need, then he arrives, he has a surprise for you—to save time he has broken the eggs in a bowl for you. You ask him how many he brought, and he replies, All of them, but I spilled some on the way over. You weigh the eggs and find that they weigh 62.1 g. Assuming that an average egg weighs 34.21 g: How much hunger is needed to react with all the eggs? How many cookies can you make? Which will you have left over, eggs or butter? How much is kit over? Relate this question to the concepts of chemical stoichiometry.
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