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Consider the reaction equilibrium, 2SO(2...

Consider the reaction equilibrium, `2SO_(2(g)) + O_(2(g))hArr , Delta H^(@) = - 198 kJ` . On the basis of Le-Chatelier's principle, the condition favourable for the forward reaction is

A

Lowering of temperature as well as pressure

B

Increasing temperature as well as pressure

C

Lowering the temperature and increasing the pressure

D

Any value of temperature and pressure

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The correct Answer is:
To determine the conditions favorable for the forward reaction in the equilibrium given by: \[ 2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)} \quad \Delta H^\circ = -198 \, \text{kJ} \] we can apply Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. ### Step 1: Identify the nature of the reaction The reaction is exothermic since the enthalpy change (\(\Delta H\)) is negative. This means that heat is released when the reaction proceeds in the forward direction. ### Step 2: Analyze the effect of temperature For an exothermic reaction: - **Decreasing the temperature** favors the forward reaction because the system will try to produce more heat to counteract the decrease. - **Increasing the temperature** favors the reverse reaction because the system will absorb the added heat. ### Step 3: Analyze the effect of pressure Next, we look at the effect of pressure on the equilibrium: - The reaction has 3 moles of gas on the reactant side (2 moles of \(SO_2\) and 1 mole of \(O_2\)) and 2 moles of gas on the product side (2 moles of \(SO_3\)). - According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, that is the product side (2 moles of \(SO_3\)). ### Step 4: Combine the effects To favor the forward reaction, we need to: 1. **Lower the temperature** (to favor the exothermic reaction). 2. **Increase the pressure** (to favor the side with fewer moles of gas). ### Conclusion The condition that is favorable for the forward reaction is **lowering the temperature and increasing the pressure**. ### Final Answer The correct condition favorable for the forward reaction is: **Lowering the temperature and increasing the pressure**. ---
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