Cosider the following reaction and determine which o fthe conditions will shift the equilibrium postion to the right ?
`4NH_(3)(g)+5O_(2)(g)hArr4NO(g)+6H_(2)O(g)+heat`

Options

A. Increasing the temperature
B. increasing the pressure
C. assigning a catalyst
D. none of above is correct

Answer

To determine which condition will shift the equilibrium position of the reaction

\[ 4 \text{NH}_3(g) + 5 \text{O}_2(g) \rightleftharpoons 4 \text{NO}(g) + 6 \text{H}_2\text{O}(g) + \text{heat} \]

to the right, we can analyze the effects of temperature, pressure, and the addition of a catalyst.

### Step-by-Step Solution:

1. **Identify the Nature of the Reaction**:
- The reaction is exothermic since heat is released. This means that the forward reaction (producing NO and H2O) releases heat.

2. **Effect of Temperature**:
- For exothermic reactions, increasing the temperature shifts the equilibrium to the left (towards the reactants) because the system will try to absorb the excess heat.
- **Conclusion**: Increasing the temperature will not shift the equilibrium to the right.

3. **Effect of Pressure**:
- According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas.
- On the reactant side, we have 4 moles of NH3 and 5 moles of O2, totaling 9 moles.
- On the product side, we have 4 moles of NO and 6 moles of H2O, totaling 10 moles.
- Since there are more moles of gas on the product side (10 moles) than on the reactant side (9 moles), increasing the pressure will shift the equilibrium to the left (towards the reactants).
- **Conclusion**: Increasing the pressure will not shift the equilibrium to the right.

4. **Effect of Adding a Catalyst**:
- A catalyst speeds up the rate of both the forward and reverse reactions equally but does not affect the position of equilibrium.
- Therefore, adding a catalyst will not shift the equilibrium position to the right or left.
- **Conclusion**: Adding a catalyst will not shift the equilibrium to the right.

5. **Final Conclusion**:
- After analyzing all the conditions, we find that none of the conditions (increasing temperature, increasing pressure, or adding a catalyst) will shift the equilibrium position to the right. Thus, the correct answer is that none of the options will shift the equilibrium to the right.