
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 4.0 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂ (g) → 2 NO₂ (g)
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- If 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 5.2 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂ (g) → 2 NO₂ (g)arrow_forwardHow many moles of NO can be produced by the reaction of 65.00 g of NH3 with 150.0 g of O2 according to the following balanced chemical equation? 4 NH3(g) + 5O2(g) → 4NO(g) + 6 H2O(g)arrow_forwardAccording to the balanced reaction below, calculate the quantity of moles of NH, gas that form when 4.20 mol of N,H, liquid completely reacts: 3 N,H,(1) → 4 NH,(g) + N,(g)arrow_forward
- How many moles of NO₂ would be produced from 4.5 mol of O₂ in the reaction below assuming the reaction has a 57.0% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)arrow_forward22.0 g of CO2 gas and 9.01 g of H2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?arrow_forwardMg(s) + 2 H2O(l) -> Mg(OH)2(aq) + H2(g) When 11.0g of Mg(s) reacts with excess water to produce 5.75g of Mg(OH)2 , what is the percent yield of the reaction?arrow_forward
- How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g) (balanced)arrow_forwardIf the percent yield for the following reaction is 75.0%, and 30.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)arrow_forwardIf 10.0 moles of O₂ are reacted with excess NO in the reaction below, and only 8.7 mol of NO₂ were collected, then what is the percent yield for the reaction? 2 NO (g) + O₂ (g) → 2 NO₂ (g)arrow_forward
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