This reaction has an equilibrium constant of Kp = 2.26 * 104 at 2...

Question

This reaction has an equilibrium constant of Kp = 2.26 * 104 at 298 K.
CO(g) + 2 H2(g) ⇌ CH3OH(g)
Calculate Kp for each reaction and predict whether reactants or
products will be favored at equilibrium. a. CH3OH(g) ⇌ CO(g) + 2 H2(g)

Accepted Answer

Hello everyone today. We're being asked to first consider the reaction of A plus B. Gives us to see and then we have a K value of 1.93 times 10 to the third power. And we're being asked to calculate K. For the reverse reaction but two times that of each reaction and product. So we're going to treat this as any other equilibrium problem in that we know that our K EQ is not going to change as we change the number of concentrations that we have. However, since we're going in the reverse and we're multiplying by two. R. K value Is going to be needed to be raised to the -2 power because we are multiplying B Products and reactions by two we must raise this equilibrium to a power and so we do -2. And so in doing this math we get 2.68 Times 10 to the -7. As our final answer. I hope this helped. And until next time.

This reaction has an equilibrium constant of Kp = 2.26 * 104 at 298 K. CO(g) + 2 H2(g) ⇌ CH3OH(g) Calculate Kp for each reaction and predict whether reactants or products will be favored at equilibrium. a. CH3OH(g) ⇌ CO(g) + 2 H2(g)

Watch next