The equilibrium constant for a reaction `A+B hArr C+D` is `1xx10^(-2)` at `298 K` and is `2` at `273 K`. The chemical process resulting in the formation of `C` and `D` is

Options

A. Exothermic
B. Endothermic
C. Unpredictable
D. There is no relationship between `DeltaH` and `K`.

Explanation

To determine whether the chemical process resulting in the formation of C and D is exothermic or endothermic, we can analyze the relationship between the equilibrium constant (K) and temperature (T) using Le Chatelier's principle.

### Step-by-Step Solution:

1. **Identify the Given Information:**
- The equilibrium constant (K) at 298 K is \(1 \times 10^{-2}\).
- The equilibrium constant (K) at 273 K is \(2\).

2. **Understand the Relationship Between Temperature and Equilibrium Constant:**
- The equilibrium constant (K) changes with temperature. For an exothermic reaction, increasing the temperature decreases K, while for an endothermic reaction, increasing the temperature increases K.

3. **Compare the Values of K at Different Temperatures:**
- At 273 K, \(K = 2\).
- At 298 K, \(K = 1 \times 10^{-2}\).
- We observe that as the temperature increases from 273 K to 298 K, the value of K decreases from 2 to \(1 \times 10^{-2}\).

4. **Interpret the Change in K:**
- Since K decreases with an increase in temperature, this indicates that the forward reaction (A + B → C + D) is exothermic. According to Le Chatelier's principle, if we increase the temperature of an exothermic reaction, the equilibrium shifts to favor the reactants (A and B), thus decreasing the value of K.

5. **Conclusion:**
- The chemical process resulting in the formation of C and D is **exothermic**.