Equilibria: compare question

Two separate gas-phase reactions are at equilibrium in closed containers at constant temperature.

Reaction 1: $\ce{N2(g) + 3H2(g) <=> 2NH3(g)}$, $\Delta H = -92.4\ \text{kJ mol}^{-1}$

Reaction 2: $\ce{H2(g) + I2(g) <=> 2HI(g)}$, $\Delta H = +9.6\ \text{kJ mol}^{-1}$

Compare the effect of increasing pressure and increasing temperature on the position of equilibrium of these two reactions. In your answer, state one similarity in the behaviour of the two equilibria under other changes in conditions.