Question

I don't understand how to solve.
1. For the exothermic reaction below, increasing the pressure would

N2(g)+3H2(g)⇄2NH3(g)
a. increase [H2]
b. increase [NH3]
c. increase [N2]
d. have no effect

2. If K=100, then the value of K for the reverse reaction is
a. the same value
b. can only be determined by experimentation
c. the negative of the value for the forward reaction
d. 0.01

Answer 1

Answer:

1. b. increase [NH3].

2. d. 0.01.

Explanation:

Hello!

In this case, for these equilibrium problems, we proceed as follows:

1. Here, we consider the Le C hatelier 's principle applied to a gas-phase reaction in which the reactants side have more number of moles; therefore, increasing the pressure will increase the products side as it has the fewest number of moles, so the answer is b. increase [NH3].

2. Here, we know that the equilibrium constant of the reverse reaction equals the inverse of the equilibrium constant of the forward reaction, thus, we obtain:

$K_{rev}=\frac{1}{K_{for}} =\frac{1}{100}=0.01$

Therefore, the answer is d. 0.01.

Best regards!