Consider the following reaction: A( g )2B( g ) Find the equilibrium partial pres

Question

Consider the following reaction:
A(g)2B(g)
Find the equilibrium partial pressures of A and B for each of the following different values of Kp . Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm . Make any appropriate simplifying assumptions

Part A Kp= 2.0

Enter your answers numerically separated by a comma. Express your answer using two significant figures

Part B

Kp= 1.8×104

Enter your answers numerically separated by a comma. Express your answer using two significant figures.

Part C

Kp= 1.6×105

Enter your answers numerically separated by a comma. Express your answer using two significant figures.

Explanation / Answer

A)

A ---> 2B

using ICE table

at equilibrium

pA = x

pB = 1 - 2x

so

Kp = [pB]^2 / [pA]

2 = (1-2x)^2 / x

2x = 1 -4x + 4x2

4x2 -6x + 1 = 0

x = 0.191

so

pA = x = 0.191 atm

pB = 1 - 2x = 0.618 atm

B)

now

1.8 * 10-4 = (1-2x)^2 / x

solving we get

x = 0.495

so

at equilibrium

pA = x = 0.495 atm

pB = 1-2x = 0.01 atm

C)

now

1.6 x 10^5 = (1-2x)^2 / x

solving we get

x = 6.25 * 10-5

so

pA = x = 6.25 * 10-5 atm

pB = 1 atm

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