Question

Consider the chemical equation in equilibrium.

Answer 1

Answer: The forward reaction will be favored.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

For the given equation:

$2H_2(g)+O_2(g)\leftrightharpoons 2H_2O(g)$

On increase of pressure

If the pressure is increased, the volume will increase according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. As the number of moles of gas molecules is lesser at the product side. So, the equilibrium will shift in the right direction or towards the products.

Thus the forward reaction will be favored.

Answer 2

Answer:

The forward reaction will be favored.

Explanation:

The reaction is:

$2H_{2}(g)+2O_{2}(g)--->2H_{2}O(g)$

As per equation (equilibrium equation), there are two moles of gaseous molecules on product side and three moles of reactant side.

a) If we increase pressure, the volume will decrease.

b) Due to decrease in volume, the moles per unit volume will increase.

c) In order to attain equilibrium again, the system will shift in the direction where it can nullify this effect [Le Chatelier's principle]

d) This can be done, if system moves in the direction where number of moles of gaseous molecules are less, which is product side.

e) Thus forward reaction will be favored.