Question

The reversible decomposition of dinitrogen tetroxide, N, O, to nitrogen dioxide, NO,, is shown. For this reaction, Keq = 0.15. = NO dinitrogen tetroxide 2NO, nitrogen dioxide At equilibrium, is the concentration of reactants or products greater? The concentration of reactants equals the concentration of products at equilibrium. The concentration of products is greater than the concentration of reactants at equilibrium. The concentration of reactants is greater than the concentration of products at equilibrium

Answer 1

Answer-

N₂O₄ $\rightleftharpoons$ 2 NO₂

K_eq = 0.15

fro a general equation,

aA + bB $\rightleftharpoons$ cC + dD

K_eq = [C]^c[D]^d/[A]^a[B]^b

applying that on the given equation,

K_eq = [NO₂]²/[N₂O₄]

Here, [N₂O₄] is the concentration of reactants while [NO₂] is the concentration of products.

Put the values,

0.15 = [NO₂]²/[N₂O₄]

0.15 = [concentration of products]²/[concentration of reactants]

From this it can be concluded that the ratio of the square of the concentration of product by the concentration of the reactants is smaller than 1.

Which means the concentration of the product is smaller than the concentration of the reactants

So, THE OPTION (The concentration of the reactants is greater than the concentration products at equillibrium) is correct.

Answer -

Given,

PCl₃ (g) + Cl₂ (g) $\rightleftharpoons$ PCl₅ (g) + heat

Shift in equilibrium when temperature is increased = ?

The heat is released is the given equation. So, the ration is exothermic reaction.

According to the Le Chatelier's principle, In an endothermic reaction raising the temperature will favour the forward reaction and in exothermic reation, raising the temperature will favour the reverse reation.

So, on increasing the temperature the equilibrium will shift toward left.

So, OPTION (Shift left) is correct.