Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g) + 6H₂O(g) 4NH,(9) + 5O₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition: compound concentration at equilibrium NO 1.4M 1.9M 0.57M 1.5M 1 H₂O NH, 0₂ Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. 0.2

Nitrogen monoxide and water react to form ammonia and oxygen, like this: 4 NO(g) + 6H₂O(g) 4NH,(9) + 5O₂(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen monoxide, water, ammonia, and oxygen has the following composition: compound concentration at equilibrium NO 1.4M 1.9M 0.57M 1.5M 1 H₂O NH, 0₂ Calculate the value of the equilibrium constant K, for this reaction. Round your answer to 2 significant digits. 0.2

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13CR

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Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: CH3OH(aq)H2CO(aq)+H2(aq) Assuming the value of K for this reaction is 3.7 1010, what are the equilibrium concentrations of each species if you start with a 1.24 M solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?
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