An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H,SO,) to form zinc sulfate (ZnSO4) and molecular hydrogen (H2). (a) Write a balanced equation for the reaction. Zn(s) + (b) How many moles are in 3.29 g of pure zinc? mol (c) How many moles of hydrogen gas are formed if one mole of zinc is treated with excess sulfuric acid? mol (d) If 3.29 g of pure Zn is treated with excess sulfuric acid, how many grams of hydrogen could be collected? g (e) If 0.0726 g of H, is obtained from 3.29 g of impure sample, what is the percent purity of the sample? 0%

An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H,SO,) to form zinc sulfate (ZnSO4) and molecular hydrogen (H2). (a) Write a balanced equation for the reaction. Zn(s) + (b) How many moles are in 3.29 g of pure zinc? mol (c) How many moles of hydrogen gas are formed if one mole of zinc is treated with excess sulfuric acid? mol (d) If 3.29 g of pure Zn is treated with excess sulfuric acid, how many grams of hydrogen could be collected? g (e) If 0.0726 g of H, is obtained from 3.29 g of impure sample, what is the percent purity of the sample? 0%

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 20CR: Solid calcium carbide (CaC2)reacts with liquid water to produce acetylene gas (C2H2)and aqueous...

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Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
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The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
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he production capacity for acrylonitrile (C3H3N)in the United States is over 2 billion pounds per year. Acrylonitrile, the building block tor acrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen: :math>2C3H6(g)+2NH3(g)+3O22C3H3N(g)+6H2O(g) l type='a'> Assuming 100% yield, determine the mass of acrylonitrile which can be produced from the mixture below: l> Mass Reactant msp;5.23102g propylene td> msp;5.00102g ammonia td> msp;1.00103g oxygen td> i>What mass of water is formed from your mixture? Calculate the mass (in grams) of each reactant after the reaction is complete.
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