Consider the following reversible reaction carried out in a sealed vessel at 25C

Question

Consider the following reversible reaction carried out in a sealed vessel at 25C A(g) + B(g) <--> 2C(g)
K=1.0 x 10^-30
When equilibrium is established ithe partial pressures of A and B are 1.2atm and 3.1atm. What is the equilibrium partial pressure of C(g)?
A. 5.2x10^-16 B. 1.9x10^-30 C. 1.9x10^-15 D. 3.7x10^-30 Consider the following reversible reaction carried out in a sealed vessel at 25C A(g) + B(g) <--> 2C(g)
K=1.0 x 10^-30
When equilibrium is established ithe partial pressures of A and B are 1.2atm and 3.1atm. What is the equilibrium partial pressure of C(g)?
A. 5.2x10^-16 B. 1.9x10^-30 C. 1.9x10^-15 D. 3.7x10^-30 A(g) + B(g) <--> 2C(g)
K=1.0 x 10^-30
When equilibrium is established ithe partial pressures of A and B are 1.2atm and 3.1atm. What is the equilibrium partial pressure of C(g)?
A. 5.2x10^-16 B. 1.9x10^-30 C. 1.9x10^-15 D. 3.7x10^-30

Explanation / Answer

Let the equilibrium partial pressure of C(g) be = Pc

The given reaction in equilibium is

A(g) + B(g) <----------> 2C(g)

at eqm: 1.2atm 3.1atm Pc atm

Given the equilibrium constant for the above reaction, K = 1.0x10-30

Hence K = 1.0x10-30 = (Pc atm)2 / (1.2atm)x(3.1atm)

=> Pc  = (3.72x10-30 )1/2  = 1.9x10-15  

Hence C is the correct answer.

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