Assume that the following chemical reaction is at equilibrium.
$$H^\circ = +26.9 \text{ kJ}$$
$$2 \text{ ICl(g)} <---> \text{ I}_2\text{(g)} + \text{ Cl}_2\text{(g)}$$
At $$25 \text{ }^\circ\text{C}$$, $$K_p = 2.0 \times 10^5$$. If the temperature is increased to $$45 \text{ }^\circ\text{C}$$, which statement applies?
a. $$K_p$$ will decrease and the reaction will proceed in the backward direction.
b. $$K_p$$ will decrease and the reaction will proceed in the forward direction.
c. $$K_p$$ will remain unchanged and the reaction will proceed in the forward direction.
d. $$K_p$$ will increase and the reaction will proceed in the backward direction.
e. $$K_p$$ will increase and the reaction will proceed in the forward direction.
O a
O b
O c
O d
O e