Increasing the pressure will _____________. 2 H Cl (g) Cl_2 (g) + H_2 (g) shift

Question

Increasing the pressure will _____________. 2 H Cl (g) Cl_2 (g) + H_2 (g) shift the reaction to the right shift the reaction to the left have no effect cannot be determined, since the temperature is unknown For the following reaction, the equilibrium constant, K_eq, is equal to 53.3. What is the concentration of I_2 at equilibrium, if the concentration of HI and H_2 are 0.212 M and 1.5756 M, respectively? H_2 + I_2 2 HI 1.576 M 0.000535 M 0.212 M 0.314 M The equilibrium constant expression for the reaction is ______________. 2 SO_3 (g) + 2 Cl_2 (g) 2 SO_2Cl_2 (g) + O_2 (g) K_eq = [SO_2Cl_2] [O_2]/[SO_3] [Cl_2] K_eq = [SO_3] [Cl_2]/[SO_2Cl_2] [O_2] K_eq = [SO_2Cl_2]^2 [O_2]/[SO_3]^2 [Cl_2]^2 K_eq = [SO_3]^2 [Cl_2]^2/[SO_2Cl_2]^2 [O_2]

Explanation / Answer

7)
increasing pressure shift the equilibrium in direction of lesser number of gaseous molecules
since number of gaseous molecules is same on both sides, there is no effect
Answer : C

8)
Keq = [HI]^2 / {[H2] [I2]}
53.3 = (0.212)^2 / {(1.576) [I2]}
[I2] = 5.35*10^-4 M
Answer: B

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