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Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at...


Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K:

2HI(g) =H2(g) +  I2(g)  

If the TEMPERATURE on the equilibrium system is suddenly decreased:

The value of Kc A. Increases
B. Decreases
C. Remains the same
The value of Qc A. Is greater than Kc
B. Is equal to Kc
C. Is less than Kc
The reaction must: A. Run in the forward direction to restablish equilibrium.
B. Run in the reverse direction to restablish equilibrium.
C. Remain the same. Already at equilibrium.
The concentration of I2 will: A. Increase.
B. Decrease.
C. Remain the same.

2)

Consider the following system at equilibrium where H° = 10.4 kJ, and Kc = 1.80×10-2, at 698 K:

2HI(g) =H2(g) +  I2(g)  

If the TEMPERATURE on the equilibrium system is suddenly increased:

The value of Kc A. Increases
B. Decreases
C. Remains the same
The value of Qc A. Is greater than Kc
B. Is equal to Kc
C. Is less than Kc
The reaction must: A. Run in the forward direction to restablish equilibrium.
B. Run in the reverse direction to restablish equilibrium.
C. Remain the same. Already at equilibrium.
The concentration of I2 will: A. Increase.
B. Decrease.
C. Remain the same.
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Answer #1

D Kc = 1.80 x 10=2 -) -ve Given: 2H₂ I (g) Hargit I2(g) A Heroin = 1024*H (endothermie T, = 698 K9 We know that Equilibrium C

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