Nitrous acid, HNO₂, can be made by reacting N₂O3 with water as depicted below in a balanced chemical equation: N₂O3 + H₂O → 2HNO₂ If 20.0 grams of N₂O3 were reacted with an excess of water and only 19.5 grams of HNO₂ actually formed, what would be the percent yield of this reaction? Molar Mass of N₂O3 = 76.01 g/mole Molar Mass HNO₂ = 47.013 g/mole Note: Give your answer in percentage, not fraction, form (e.g if it were 25.4%, enter 25.4, NOT 0.254) PLEASE CLEARLY SHOW YOUR WORK FOR THIS AND SUBMIT IT

Nitrous acid, HNO₂, can be made by reacting N₂O3 with water as depicted below in a balanced chemical equation: N₂O3 + H₂O → 2HNO₂ If 20.0 grams of N₂O3 were reacted with an excess of water and only 19.5 grams of HNO₂ actually formed, what would be the percent yield of this reaction? Molar Mass of N₂O3 = 76.01 g/mole Molar Mass HNO₂ = 47.013 g/mole Note: Give your answer in percentage, not fraction, form (e.g if it were 25.4%, enter 25.4, NOT 0.254) PLEASE CLEARLY SHOW YOUR WORK FOR THIS AND SUBMIT IT

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 7RQ: Consider the hypothetical reaction between A2 and AB pictured below. What is the balanced equation?...

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When potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?
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4.72 The picture shown depicts the species present at the start of a combustion reaction between methane, CH4 and oxygen, O2 (a) What is the limiting reactant? (b) Draw the resulting state after this set of reactants has reacted as far as possible.
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
A power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.
4.69 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. 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.
The space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.
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