Reaction X has a forward activation energy of 82 kJ/mol and Δ H = +36 kJ/mol…

Step 1. Reaction X. It is endothermic. $E_a' = 82 - (+36) = 46\ \text{kJ/mol}$. The products are higher than the reactants, so the way back is shorter.

Step 2. Reaction Y. It is exothermic. $E_a' = 57 - (-48) = 105\ \text{kJ/mol}$. The products are lower, so the way back is longer.

Step 3. The faster forward step. Y has the lower forward barrier, $57\ \text{kJ/mol}$ against $82\ \text{kJ/mol}$. With the same $A$ and $T$, $e^{-E_a/RT}$ is larger for Y, so Y is faster.