For the reactionH₂(e) + CO₂(e) H₂O(g) + CO(e)at 700 °C, K, -0.534. Calculate the number of moles of H, that are present at equilibrium if a mixture of 0.420 mole of CO and 0.420 mole of H₂O is heatedto 700 °C in a 60.0 L container. Round your answer to 3 significant digitsmolD.PX4

Given:Reaction: Kc at 7000C , Equilibrium constant Kc= 0.534Initial moles of CO=0.420 molesInitial…

For the reaction H₂(e) + CO₂(e) H₂0(e) + сo(e) at 700 "C, K, -0.534. Calculate the number of moles of H, that are present at equilibrium f a mixture of 0.420 mole of CO and 0.420 mole of H₂O is heated to 700 °C in a 60.0 L container Round your answer to 3 significant digits OP X

For the reaction H₂(e) + CO₂(e) H₂0(e) + сo(e) at 700 "C, K, -0.534. Calculate the number of moles of H, that are present at equilibrium f a mixture of 0.420 mole of CO and 0.420 mole of H₂O is heated to 700 °C in a 60.0 L container Round your answer to 3 significant digits OP X

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 3RQ

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Question

For the reaction
H₂(e) + CO₂(e) H₂O(g) + CO(e)
at 700 °C, K, -0.534. Calculate the number of moles of H, that are present at equilibrium if a mixture of 0.420 mole of CO and 0.420 mole of H₂O is heated
to 700 °C in a 60.0 L container. Round your answer to 3 significant digits
mol
D.P
X
4

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Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
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