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Chemistry: An Atoms First Approach

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 8RQ

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What is the maximum mass of S, that can be produced by combining 81.0 g of each reactant?
8 SO, + 16H,S -
3 Sg + 16 H,O
mass of Sg:
g

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Consider the following mixture of SO2(g) and O2(g). If SO2(g) and O2(g) react to form SO3(g), draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If 96.0 g of SO2 react with 32.0 g O2, what mass o f product will form?
Phosphine gas reacts with oxygen according to the following equation: 4PH3(g)+8O2(g)P4O10(s)+6H2O(g) Calculate (a) the mass of tetraphosphorus decaoxide produced from 12.43 mol of phosphine. (b) the mass of PH3 required to form 0.739 mol of steam. (c) the mass of oxygen gas that yields 1.000 g of steam. (d) the mass of oxygen required to react with 20.50 g of hosphine.
For the following reactions, write the ratios that can be established among molar amounts of the various compounds. 2H2+O22H2O 2H2O22H2O+O2 P4+5O2P4O10 2KClO32KCl+3O2 xs
4.45 If 21 g of H2S is mixed with 38 g of O2 and 31 g of SO2 forms, what is the percentage yield? 2H2S+3O22SO2+2H2O
4.41 The percentage yield of the following reaction is consistently 87%. CH4(g)+4S(g)CS2(g)+2H2S(g) How many grams of sulfur would be needed to obtain 80.0 g of CS2?
The reaction of methane and water is one way to prepare hydrogen for use as a fuel: CH4(g) + H2O(g) CO(g) + 3 H2(g) If this reaction has a 37% yield under certain conditions, what mass of CH4 is required to produce 15 g of H2?
A reaction of 43.1 g CS2 with excess Cl2 yields 45.2 g CCl4 and 41.3 g S2Cl2. What is the percent yield of each product?
Over the years, the thermite reaction has been used for welding railroad rails, in incendiary bombs, and to ignite solid-fuel rocket motors. The reaction is Fe2O3(s)+2Al(s)2Fe(l)+Al2O3(s) What masses of iron(III) oxide and aluminum must be used to produce 15.0 g iron? What is the maximum mass of aluminum oxide that could be produced?
One mol of ammonia reacts with 1.00 mol of oxygen to form nitrogen oxide and water according to the reaction 4NH3(g)+5O2(g)4NO(g)+6H2O(l)State which statements are true about the reaction and make the false statements true. (a) All the oxygen is consumed. (b) 4.00 mol NO are produced. (c) 1.50 mol H2O are produced. (d) The description of the experiment does not provide enough information to determine percent yield. (e) Three moles of water are produced for every two moles of NO obtained.
In Example 4.2, you found that a particular mixture of CO and H2 could produce 407 g CH3OH. CO(g) + 2H2(g) CH3OH (l) If only 332 g of CH3OH is actually produced, what is the percent yield of the compound?
Consider the following diagram, where atom X is represented by a square and atom Y is represented by a circle. (a) Write the equation for the reaction represented by the diagram. (b) If each circle stands for a mole of Y and each square a mole of X, how many moles of X did one start with? How many moles of Y? (c) Using the same representation described in part (b), how many moles of product are formed? How many moles of X and Y are left unreacted?
Citric acid, C6H5CH3, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger . The equation representing this reaction is C12H22O11+H2O+3O22C6H8O7+4H2O What mass of citric acid is produced from exactly 1 metric ton (1.000103kg) of sucrose if the yield is 92.30%?

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