In which direction is equilibrium expected to shift on increasing temperature in the following reactions ?
` 2CO_2 (g) hArr 2CO(g)+ O_2(g), `
` " " Delta H =+ 212. 8 " kcal " `

Answer

To determine the direction in which the equilibrium will shift upon increasing the temperature for the given reaction, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction and Its Nature**:
The given reaction is:
\[ 2CO_2 (g) \rightleftharpoons 2CO(g) + O_2(g) \]
The enthalpy change (\(\Delta H\)) is given as \(+212.8 \, \text{kcal}\), indicating that the reaction is endothermic.

2. **Understand the Implications of \(\Delta H\)**:
Since \(\Delta H\) is positive, it means that heat is absorbed during the reaction. In an endothermic reaction, the reactants require heat to convert into products.

3. **Apply Le Chatelier's Principle**:
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to counteract that change and establish a new equilibrium.

4. **Analyze the Effect of Increasing Temperature**:
- For endothermic reactions, increasing the temperature favors the formation of products because the system will try to absorb the added heat.
- In this case, since the reaction absorbs heat, increasing the temperature will shift the equilibrium to the right (towards the products).

5. **Conclusion**:
Therefore, upon increasing the temperature, the equilibrium will shift to the right, favoring the formation of \(2CO(g) + O_2(g)\).

### Final Answer:
The equilibrium is expected to shift to the right (towards the products) upon increasing the temperature.

---