Question

1. Question 22

   1 Point

   Consider the equilibrium below:

   2 NO (g) + Cl₂ (g) <--> 2 NOCl (g)    K_p = 6.50 x 10⁴ at 308 K

   BLANK-1 Does the equilibrium favour the reactants or products at 308K? (insert appropriate term)

   BLANK-2 Does entropy increase, decrease or remain unchanged as reactants convert to products? (insert appropriate term)

   • BLANK-1
   • BLANK-2

Answer 1

1) As the equilibrium constant is greater than 1 (i.e. Kp = 6.50 x 10⁴) at 308 K then the equilibrium favor the products. The solution mixture contain products.

Because , Kp = [products]ⁿ/[reactants]^m

When Kp >> 1 this shows that products are large in number than the reactants.

2) Increase in the entropy increases the product formation from reactants. Entropy is measure of disorderness.

This shows that change in the enthalpy is greater than 1 i.e. increase in entropy. $\Delta$ S >>1

$\Delta$S = change in entropy = n$\Sigma$Sproducts - n$\Sigma$Sreactants

$\Delta$S is greater than 1 only when entropy of products is greater than entropy of reactants.