Nitric oxide, NO, is a product generated in automobile exhaust. What mass of NO (30.01 g/mol) can be formed from the reaction of 2.00 g NO2 (46.01 g/mol) and excess oxygen according to the equation shown below? NO2(g) + O2(g) –→ NO(g) + O3(g) O 0.769 g NO O 3.07 g NO O 15.00 g NO O 2.00 g NO O 1.30 g NO
Nitric oxide, NO, is a product generated in automobile exhaust. What mass of NO (30.01 g/mol) can be formed from the reaction of 2.00 g NO2 (46.01 g/mol) and excess oxygen according to the equation shown below? NO2(g) + O2(g) –→ NO(g) + O3(g) O 0.769 g NO O 3.07 g NO O 15.00 g NO O 2.00 g NO O 1.30 g NO
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 8PS
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Transcribed Image Text:Nitric oxide, NO, is a product generated in automobile exhaust. What mass of NO (30.01 g/mol) can be formed from the reaction of 2.00 g NO2 (46.01 g/mol) and excess
oxygen according to the equation shown below?
NO2(g) + O2(g) –→ NO(g) + O3(g)
O 0.769 g NO
O 3.07 g NO
O 15.00 g NO
O 2.00 g NO
O 1.30 g NO
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Question 23
Consider the balanced equation shown below. How many moles of KCIO3 would be required to produce 15.45 moles of O2?
2KCIO3(s) → 2KCI(s) + 302(g)
O 7.725 moles O2
O 10.30 moles O2
O 30.90 moles O2
O 23.18 moles O2
O 15.45 moles O2
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