# Problem: The reaction below has an equilibrium constant Kp=2.2×106 at 298 K.  2COF2(g) ⇌ CO2(g) + CF4(g)a. Calculate Kp for the reaction 4COF2(g) ⇌ 2CO2(g) + 2CF4(g). Express your answer using two significant figures.b. Predict whether reactants or products will be favored at equilibrium in the equation above.c. Calculate Kp for the reaction below. Express your answer using two significant figures.     2/3 COF2(g) ⇌ 1/3 CO2(g) + 1/3 CF4(g) d. Predict whether reactants or products will be favored at equilibrium in the equation above.e. Calculate Kp for the reaction below. Express your answer using two significant figures.     2CO2(g) + 2CF4(g) ⇌ 4COF2(g) f. Predict whether reactants or products will be favored at equilibrium in the equation above.

🤓 Based on our data, we think this question is relevant for Professor Brown's class at HOWARDCC.

###### FREE Expert Solution

We are given the following reaction:

2 COF2(g) ⇌ CO2(g) + CF4(g)           Kp at 298 K: 2.2×106

A. We are asked to calculate Kp for the reaction

4 COF2(g) ⇌ 2 CO2(g) + 2 CF4(g)

Recall: Reversing a reaction gives us the reciprocal of K, while multiplying a reaction by a value makes it the power for K. The reaction was multiplied by 2, hence we have:

${\left({K}_{p}\right)}^{\mathbf{n}}\mathbf{=}{\left(2.2×{10}^{6}\right)}^{\mathbf{2}}\mathbf{=}$4.84×1012

###### Problem Details

The reaction below has an equilibrium constant Kp=2.2×106 at 298 K.

2COF2(g) ⇌ CO2(g) + CF4(g)

a. Calculate Kp for the reaction 4COF2(g) ⇌ 2CO2(g) + 2CF4(g). Express your answer using two significant figures.

b. Predict whether reactants or products will be favored at equilibrium in the equation above.

c. Calculate Kp for the reaction below. Express your answer using two significant figures.

2/3 COF2(g) ⇌ 1/3 CO2(g) + 1/3 CF4(g)

d. Predict whether reactants or products will be favored at equilibrium in the equation above.

e. Calculate Kp for the reaction below. Express your answer using two significant figures.

2CO2(g) + 2CF4(g) ⇌ 4COF2(g)

f. Predict whether reactants or products will be favored at equilibrium in the equation above.