Given the reaction: CO(NH2),(s) + H,O(g) = CO₂(g) + 2 NH3(g) Kp = 1.39 at 500 K If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be -- A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase. This means that: The value of K, for the given reaction at 600 K is The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is [.
Given the reaction: CO(NH2),(s) + H,O(g) = CO₂(g) + 2 NH3(g) Kp = 1.39 at 500 K If this reaction system is initially at equilibrium and a catalyst is added, the new position of equilibrium will be -- A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase. This means that: The value of K, for the given reaction at 600 K is The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is [.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Given the reaction:
CO(NH2),(s) + H2O(g) = CO2(9) + 2NH3(g)
--
Kp
If this reaction system is initially at equilibrium and a catalyst is added, the new position of
equilibrium will be
= 1.39 at 500 K
The value of K, for the given reaction at 600 K is
The reaction CO(NH₂)₂(s) + H₂O(g) → CO₂(g) + 2 NH₂(g) is --
A flask containing CO₂(g), NH₂(g), CO(NH₂)₂(s) and H₂O(g) is initially at equilibrium at 500 K. When the flask is
heated to 600 K, the amounts of CO(NH₂)₂(s) and H₂O(g) decrease and the amounts of CO₂(g) and NH₂(g) increase.
This means that:
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