Consider the hypothetical reaction A(g)←→2B(g). A flask is charged with 0.77 atm of pure A, after which it is allowed to reach equilibrium at 0 ∘C. At equilibrium the partial pressure of A is 0.35 atm .A: What is the total pressure in the flask at equilibrium?
B:What is the value of Kp?

For A: The total pressure in the flask at equilibrium is 1.19 atm

For B: The value of for the given equation is 2.016

Explanation:

We are given:

Initial partial pressure of A = 0.77 atm

Equilibrium partial pressure of A = 0.35 atm

For the given chemical equation:

Initial:         0.77

At eqllm:   0.77-x     2x

Evaluating the value of 'x'

Equilibrium partial pressure of B = 2x = (2 × 0.42) = 0.84 atm

Total pressure in the flask at equilibrium =

Hence, the total pressure in the flask at equilibrium is 1.19 atm

The expression of for given equation follows:

Putting values in above expression, we get:

Hence, the value of for the given equation is 2.016

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