Problem: At 700 K, the reaction below has an Kp value of 54. An equilibrium mixture at this temperature was found to contain 0.712 atm of H2 and 2.77 atm of HI. Calculate the equilibrium pressure of I2.H2(g) + I2(g) <=> 2 HI(g). Enter to 2 decimal place.a. 0.07 atmb. 0.20 atmc. 581.93 atmd. 19.95 atme. 210.08 atm

FREE Expert Solution

We’re being asked to calculate the equilibrium concentration of I2, given the following reaction:

H2(g) + I2(g) ⇌ 2 HI(g).;  Kp = 54


We're given the equilibrium pressures:

PH2 = 0.712 atm
PI2 = ?
PHI = 2.77 atm


The Kp expression for the reaction is:

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Problem Details

At 700 K, the reaction below has an Kp value of 54. An equilibrium mixture at this temperature was found to contain 0.712 atm of H2 and 2.77 atm of HI. Calculate the equilibrium pressure of I2.

H2(g) + I2(g) <=> 2 HI(g). Enter to 2 decimal place.

a. 0.07 atm
b. 0.20 atm
c. 581.93 atm
d. 19.95 atm
e. 210.08 atm

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