Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80x10-2, at 698 K. %3D 2HI(g) H2(g) + I(g) When 0.23 moles of H2(g) are added to the equilibrium system at constant temperature: The value of K. The value of Q. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of I, will Submit Answer Retry Entire Group 4 more group attempts remaining <>
Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80x10-2, at 698 K. %3D 2HI(g) H2(g) + I(g) When 0.23 moles of H2(g) are added to the equilibrium system at constant temperature: The value of K. The value of Q. The reaction must Orun in the forward direction to restablish equilibrium. Orun in the reverse direction to restablish equilibrium. remain the same. It is already at equilibrium. The concentration of I, will Submit Answer Retry Entire Group 4 more group attempts remaining <>
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.98PAE
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Question
![Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10, at 698 K.
2HI(g)
H2(g) + I(g)
When 0.23 moles of H2(g) are added to the equilibrium system at constant temperature:
The value of K.
The value of Q.
K.
The reaction must
Orun in the forward direction to restablish equilibrium.
run in the reverse direction to restablish equilibrium.
remain the same. It is already at equilibrium.
The concentration of I, will
Submit Answer
Retry Entire Group
4 more group attempts remaining](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9c89e543-4ffd-4c36-8dc6-0952cfcad04e%2F20f34e76-5773-4295-8444-2b0690192ce6%2F78ghgzk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10, at 698 K.
2HI(g)
H2(g) + I(g)
When 0.23 moles of H2(g) are added to the equilibrium system at constant temperature:
The value of K.
The value of Q.
K.
The reaction must
Orun in the forward direction to restablish equilibrium.
run in the reverse direction to restablish equilibrium.
remain the same. It is already at equilibrium.
The concentration of I, will
Submit Answer
Retry Entire Group
4 more group attempts remaining
Expert Solution
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Step 1: Given
Given:
∆H° = 10.4 KJ
Kc = 1.80 × 10-2
Tempreture = 698 K
Reaction:
2HI(g) <=> H2(g) + I2(g)
Moles of H2 added = 0.23 moles
Value of Kc = ?
Value of Qc = ?
Reaction must = ?
Concentration of I2 = ?
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