Question 15 If \( K_c = 2.44 \times 10^{-3} \) for the reaction: \[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \, \text{SO}_3(g) \, \text{at} \, 700^\circ \text{C}, \] then \( K_p = \) - \( 8.56 \times 10^{-7} \) - \( 9.50 \times 10^{-6} \) - \( 8.66 \times 10^{-5} \) - \( 4.88 \times 10^{-6} \) - \( 6.87 \times 10^{-2} \) *Note: Shifting to another question will save this response.*
Question 15 If \( K_c = 2.44 \times 10^{-3} \) for the reaction: \[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \, \text{SO}_3(g) \, \text{at} \, 700^\circ \text{C}, \] then \( K_p = \) - \( 8.56 \times 10^{-7} \) - \( 9.50 \times 10^{-6} \) - \( 8.66 \times 10^{-5} \) - \( 4.88 \times 10^{-6} \) - \( 6.87 \times 10^{-2} \) *Note: Shifting to another question will save this response.*
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 102QRT
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![Question 15
If \( K_c = 2.44 \times 10^{-3} \) for the reaction:
\[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \, \text{SO}_3(g) \, \text{at} \, 700^\circ \text{C}, \]
then \( K_p = \)
- \( 8.56 \times 10^{-7} \)
- \( 9.50 \times 10^{-6} \)
- \( 8.66 \times 10^{-5} \)
- \( 4.88 \times 10^{-6} \)
- \( 6.87 \times 10^{-2} \)
*Note: Shifting to another question will save this response.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd523b0c2-1906-4841-b390-7c0a9a379a7e%2F4998cac2-3b9a-4529-bdd2-7f7873acb8dc%2Fnw8vxbj_processed.png&w=3840&q=75)
Transcribed Image Text:Question 15
If \( K_c = 2.44 \times 10^{-3} \) for the reaction:
\[ 2 \, \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \, \text{SO}_3(g) \, \text{at} \, 700^\circ \text{C}, \]
then \( K_p = \)
- \( 8.56 \times 10^{-7} \)
- \( 9.50 \times 10^{-6} \)
- \( 8.66 \times 10^{-5} \)
- \( 4.88 \times 10^{-6} \)
- \( 6.87 \times 10^{-2} \)
*Note: Shifting to another question will save this response.*
Expert Solution
Step 1
Relation between Kp and Kc:
Kp = Kc (RT)∆n
Where, ∆n = Number of product molecules - Number of reactant molecules
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