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PRACTICE EXAMPLE A: potassium chlorate? How many moles of O₂ are produced from the decomposition of 1.76 moles of 2 KCIO3(s) →→→2 KCl(s) + 3 O₂(g) PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag₂O(s) 4 Ag(s) + O₂(g)

PRACTICE EXAMPLE A: potassium chlorate? How many moles of O₂ are produced from the decomposition of 1.76 moles of 2 KCIO3(s) →→→2 KCl(s) + 3 O₂(g) PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag₂O(s) 4 Ag(s) + O₂(g)

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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PRACTICE EXAMPLE A: potassium chlorate? How many moles of O₂ are produced from the decomposition of 1.76 moles of

2 KCIO3(s) →→→2 KCl(s) + 3 O₂(g)

PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide?

2 Ag₂O(s) 4 Ag(s) + O₂(g)

 

EXAMPLE 4-2 Relating the Numbers of Moles of Reactant and Product How many moles of CO2 are produced in the combustion of 2.72 mol of triethylene glycol, C,H1404, in an excess of O,? Analyze "An excess of O," means that there is more than enough O2 available to permit the complete conversion of the triethylene glycol to CO2 and H20. The factor for converting from moles of C,H14O4 to moles of CO2 is obtained from the balanced equation for the combustion reaction. Solve The first step in a stoichiometric calculation is to write a balanced equation for the reaction. The balanced chemical equation for the reaction is given below. 2 C,H14O4 + 15 O2 → 12 CO2 + 14 H20 Thus, 12 mol CO2 are produced for every 2 mol C,H14O4 burned. The production of 12 mol CO2 is equivalent to the consumption of 2 mol C,H14O4; thus, the ratio 12 mol CO2/2 mol C,H1404 converts from mol C,H1404 to mol CO2. 12 mol CO2 ? mol CO2 = 2.72 mol CgH14O4 × = 16.3 mol CO2 2 mol C6H1404 Assess The expression above can be written in terms of two equal ratios: ? mol CO2 12 mol CO2 2.72 mol C,H14O4 2 mol C,H1404 You may find it easier to set up an expression in terms of ratios and then solve it for the unknown quantity. PRACTICE EXAMPLE A: How many moles of O2 are produced from the decomposition of 1.76 moles of potassium chlorate? 2 KCIO3(s) 2 KCI(s) + 3 O2(g) - PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag20(s) 4 Ag(s) + O2(g) >
Transcribed Image Text:EXAMPLE 4-2 Relating the Numbers of Moles of Reactant and Product How many moles of CO2 are produced in the combustion of 2.72 mol of triethylene glycol, C,H1404, in an excess of O,? Analyze "An excess of O," means that there is more than enough O2 available to permit the complete conversion of the triethylene glycol to CO2 and H20. The factor for converting from moles of C,H14O4 to moles of CO2 is obtained from the balanced equation for the combustion reaction. Solve The first step in a stoichiometric calculation is to write a balanced equation for the reaction. The balanced chemical equation for the reaction is given below. 2 C,H14O4 + 15 O2 → 12 CO2 + 14 H20 Thus, 12 mol CO2 are produced for every 2 mol C,H14O4 burned. The production of 12 mol CO2 is equivalent to the consumption of 2 mol C,H14O4; thus, the ratio 12 mol CO2/2 mol C,H1404 converts from mol C,H1404 to mol CO2. 12 mol CO2 ? mol CO2 = 2.72 mol CgH14O4 × = 16.3 mol CO2 2 mol C6H1404 Assess The expression above can be written in terms of two equal ratios: ? mol CO2 12 mol CO2 2.72 mol C,H14O4 2 mol C,H1404 You may find it easier to set up an expression in terms of ratios and then solve it for the unknown quantity. PRACTICE EXAMPLE A: How many moles of O2 are produced from the decomposition of 1.76 moles of potassium chlorate? 2 KCIO3(s) 2 KCI(s) + 3 O2(g) - PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag20(s) 4 Ag(s) + O2(g) >
PRACTICE EXAMPLE A: How many moles of O2 are produced from the decomposition of 1.76 moles of potassium chlorate? 2 KCIO3(s) 2 KCI(s) + 3 O2(g) PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag20(s) 4 Ag(s) + O2(g) -
Transcribed Image Text:PRACTICE EXAMPLE A: How many moles of O2 are produced from the decomposition of 1.76 moles of potassium chlorate? 2 KCIO3(s) 2 KCI(s) + 3 O2(g) PRACTICE EXAMPLE B: How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide? 2 Ag20(s) 4 Ag(s) + O2(g) -
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