For the reaction 2HI (g) H_2 (g) + I_2 (g), K_c = 0.290 at 400 K. If the initial

Q: For the reaction 2HI (g) H_2 (g) + I_2 (g), K_c = 0.290 at 400 K. If the initial

Qc = [H2][I2]/[HI]^2 = (1.50*10^-3)*(1.50*10^-3)/ (4.0*10^-3)^2 = 0.1406 Kc = 0.2990 Since Qc < Kc, the reaction is moving to product side So, concentration of product will increase and that of reactant will decrease Answer: b

ID: 512596 • Letter: F

Question

For the reaction 2HI (g) H_2 (g) + I_2 (g), K_c = 0.290 at 400 K. If the initial concentration of HI is 4.0 times 10^-3M and the initial concentrations of H_2, and I_2 are both 1.50 times 10^- 3M at 400 K, which one of the following statements is correct? Select one The concentrations of HI and I_2 will increase as the system is approaching equilibrium The concentrations of H_2 and I_2 will increase as the system is approaching equilibrium. The system is at equilibrium. The concentrations of H_2 and HI will decrease as the system is approaching equilibrium. The concentration of HI will increase as the system is approaching equilibrium.

Explanation / Answer

Qc = [H2][I2]/[HI]^2

= (1.50*10^-3)*(1.50*10^-3)/ (4.0*10^-3)^2

= 0.1406

Kc = 0.2990

Since Qc < Kc, the reaction is moving to product side

So, concentration of product will increase and that of reactant will decrease

Answer: b

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For the reaction 2HI(g) H2(g) + I2(g), Kc = 0.290 at 400 K. If the initial conce

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For the reaction 2HI (g) H_2 (g) + I_2 (g), K_c = 0.290 at 400 K. If the initial

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