1. One process to make molecular hydrogen gas passes hot steam over graphite to create a mixture of carbon monoxide and hydrogen. C(s, graphite) + H20(g) = CO(g) + H2(g) K, = 28.3 What will be the equilibrium partial pressures of H,O(g) and H;lg) if the reaction mixture initially only contains water vapor at a pressure of 7.65 atm and an excess of graphite? 2. Ammonia reacts with water to produce ammonium ion and hydroxide ion as shown in the equation below. NH3(aq) + H20(1) = NH; (aq) + OH¯(aq) Ke = 1.79 x 10-5 If the reaction mixture initially only contains 0.255 M NH, and water, what will be the equilibrium concentrations of NH;(aq) and NH, (aq)?
1. One process to make molecular hydrogen gas passes hot steam over graphite to create a mixture of carbon monoxide and hydrogen. C(s, graphite) + H20(g) = CO(g) + H2(g) K, = 28.3 What will be the equilibrium partial pressures of H,O(g) and H;lg) if the reaction mixture initially only contains water vapor at a pressure of 7.65 atm and an excess of graphite? 2. Ammonia reacts with water to produce ammonium ion and hydroxide ion as shown in the equation below. NH3(aq) + H20(1) = NH; (aq) + OH¯(aq) Ke = 1.79 x 10-5 If the reaction mixture initially only contains 0.255 M NH, and water, what will be the equilibrium concentrations of NH;(aq) and NH, (aq)?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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please explain as doing it. thanks
![**Chemical Equilibrium Problems**
1. **Hydrogen Production via Graphite Reaction**
One process to make molecular hydrogen gas involves passing hot steam over graphite to create a mixture of carbon monoxide and hydrogen. The chemical reaction is represented by:
\[
C(s, \text{graphite}) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)
\]
The equilibrium constant (\(K_p\)) for this reaction is 28.3.
*Problem:*
What will be the equilibrium partial pressures of \(H_2O(g)\) and \(H_2(g)\) if the reaction mixture initially only contains water vapor at a pressure of 7.65 atm and an excess of graphite?
2. **Ammonia Reaction with Water**
Ammonia reacts with water to produce ammonium ion and hydroxide ion as shown in the equation below:
\[
NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq) \quad K_c = 1.79 \times 10^{-5}
\]
*Problem:*
If the reaction mixture initially only contains 0.255 M \(NH_3\) and water, what will be the equilibrium concentrations of \(NH_3(aq)\) and \(NH_4^+(aq)\)?
**Note:** There are no graphs or diagrams associated with this text. The problems focus on calculating equilibrium positions for specified chemical reactions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb4bda451-1bcc-473c-9a91-77116df85d00%2F1ee84e5d-a814-4a70-a90e-38024210d8d3%2Fg6uitp5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium Problems**
1. **Hydrogen Production via Graphite Reaction**
One process to make molecular hydrogen gas involves passing hot steam over graphite to create a mixture of carbon monoxide and hydrogen. The chemical reaction is represented by:
\[
C(s, \text{graphite}) + H_2O(g) \rightleftharpoons CO(g) + H_2(g)
\]
The equilibrium constant (\(K_p\)) for this reaction is 28.3.
*Problem:*
What will be the equilibrium partial pressures of \(H_2O(g)\) and \(H_2(g)\) if the reaction mixture initially only contains water vapor at a pressure of 7.65 atm and an excess of graphite?
2. **Ammonia Reaction with Water**
Ammonia reacts with water to produce ammonium ion and hydroxide ion as shown in the equation below:
\[
NH_3(aq) + H_2O(l) \rightleftharpoons NH_4^+(aq) + OH^-(aq) \quad K_c = 1.79 \times 10^{-5}
\]
*Problem:*
If the reaction mixture initially only contains 0.255 M \(NH_3\) and water, what will be the equilibrium concentrations of \(NH_3(aq)\) and \(NH_4^+(aq)\)?
**Note:** There are no graphs or diagrams associated with this text. The problems focus on calculating equilibrium positions for specified chemical reactions.
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