For the reaction 2 S2O (g) + 5 Ch (g) rightarrow 4 SO3 (g) and K. = 3.25* 10-3 a

Q: For the reaction 2 S2O (g) + 5 Ch (g) rightarrow 4 SO3 (g) and K. = 3.25* 10-3 a

2s2o(g) + 5 o2(g) -----> 4 so3(g) k = 3.25*10^(-3) initial concentrations S2O = 0.1 M O2 = 1.5 M SO3 = 0.05 M Reaction queotient = [SO3]^4/[O2]^5[S2O]^2 = (0.05^4)/((1.5^5)(0.1^2)) = 8.23*10^-5 M q

ID: 887881 • Letter: F

Question

For the reaction 2 S2O (g) + 5 Ch (g) rightarrow 4 SO3 (g) and K. = 3.25* 10-3 and initial concentrations: S2O = 0.100M O2 = 1.50 M rightarrow SO3 = 0.0500 M Which statement is correct? Q = 8.23 * 10-5 and the reaction must shift to the left to reach equilibrium Q = 8.23 * 10-5 and the reaction must shift to the right to reach equilibrium Q = 12200 and the reaction must shift to the right to reach equilibrium Q = 3.33 and the reaction must shift to the left to reach equilibrium Q = 3.33 and the reaction must shift to the right to reach equilibrium

Explanation / Answer

2s2o(g) + 5 o2(g) -----> 4 so3(g) k = 3.25*10^(-3)

initial concentrations

S2O = 0.1 M O2 = 1.5 M SO3 = 0.05 M

Reaction queotient = [SO3]^4/[O2]^5[S2O]^2

= (0.05^4)/((1.5^5)(0.1^2))

= 8.23*10^-5 M

q<k so that equilibrium shifts to the right to reach equilibrium.

answer : B is correct.

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For the reaction 2 S2O (g) + 5 Ch (g) rightarrow 4 SO3 (g) and K. = 3.25* 10-3 a

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