Statement 1: The equilibrium constant may show higher or lower values with increase in temperature Statement 2: The change depends on the heat of reaction at equilibrium.

Question

Statement 1: The equilibrium constant may show higher or lower values with increase in temperature Statement 2: The change depends on the heat of reaction at equilibrium. (A) If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation o f the statement 1 . (B) Ifboth Statement 1 and Statement 2 are true but statement 2 is not the correct explanation o f the statement 1 . (C) If Statement 1 is true but Statement 2 is false. (D) If Statement 1 is false but Statement 2 is true.

Tardigrade Admin · Accepted Answer

2.303 log (Kc2/Kc1)=(Δ H/R)([T2-T1]/T1T2); if Δ H=-ve, Kc2 < Kc1 if Δ H=+ve, Kc2 > Kc1.

Q. Statement 1: The equilibrium constant may show higher or lower values with increase in temperature
Statement 2: The change depends on the heat of reaction at equilibrium.

If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation o f the statement 1 .

Ifboth Statement 1 and Statement 2 are true but statement 2 is not the correct explanation o f the statement 1 .

If Statement 1 is true but Statement 2 is false.

If Statement 1 is false but Statement 2 is true.

$2.303 l o g \frac{K _{c_{2}}}{K _{c_{1}}} = \frac{Δ H}{R} \frac{[ T _{2} - T _{1} ]}{T _{1} T _{2}};$
if $Δ H = - v e, K_{c_{2}} < K_{c_{1}}$ if $Δ H = + v e, K_{c_{2}} > K_{c_{1}} .$

Q. Statement 1: The equilibrium constant may show higher or lower values with increase in temperature Statement 2: The change depends on the heat of reaction at equilibrium.