Question

$\begin{array}{cccccc}& \text{List A}& & \text{List B}& & \text{List C}\\ A.& \text{Rate of reaction}& 1.& -\frac{\Delta \left[A\right]}{\Delta t}=-\frac{d\left[A\right]}{dt}& a.& \Delta H=\text{+ ve}\\ B.& \text{Rate constant of a reaction}& 2.& V_t=V_0& b.& \Delta H=-ve\\ C.& \text{Equilibrium constant}& 3.& V_t\ne V_0& c.& t\to 0\\ D.& V_t=\frac{V_0.t}{273}& 4.& \text{Increases}& d.& \Delta H\to 0\\ E.& V_t=V_0+\frac{V_0.t}{273}& 5.& \text{Decreases}& e.& T\to 0\end{array}$

Upon increasing temperature,

• A. C - 4 - c
• B. C - 3 - c
• C. C - 4 - d
• D. C - 5 - b

Answer 1

The correct option is D

C - 5 - b

When temperature is increased:

For an exothermic reaction - equilibrium constant falls

For an endothermic reaciton - equilibrium constant increases