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aA+bBhArrcC+dD In above reaction low p...

`aA+bBhArrcC+dD`
In above reaction low pressure and high temperature, conditions are shift equilibrium in back direction so correct set:

A

`(a+b)gt(c+d),DeltaHgt0`

B

`(a+b)lt(c+d),DeltaHgt0`

C

`(a+b)lt(c+d),DeltaHlt0`

D

`(a+B)gt(c+d),DeltaHlt0`

Text Solution

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The correct Answer is:
To solve the question regarding the equilibrium reaction \( aA + bB \rightleftharpoons cC + dD \) under low pressure and high temperature conditions, we will analyze how these conditions affect the equilibrium position. ### Step-by-step Solution: 1. **Understand the Reaction**: The equilibrium reaction is given as \( aA + bB \rightleftharpoons cC + dD \). Here, \( A \) and \( B \) are the reactants, while \( C \) and \( D \) are the products. 2. **Identify the Conditions**: The question specifies low pressure and high temperature. We need to determine how these conditions affect the equilibrium position. 3. **Effect of Low Pressure**: According to Le Chatelier's principle, if the pressure is decreased, the equilibrium will shift towards the side with more moles of gas. In this case, if \( a + b > c + d \) (more moles of reactants than products), the equilibrium will shift to the left (backward direction). 4. **Effect of High Temperature**: For exothermic reactions, increasing the temperature shifts the equilibrium to the left (backward direction) as the system tries to absorb the added heat. Conversely, for endothermic reactions, increasing temperature shifts the equilibrium to the right (forward direction). 5. **Determine the Type of Reaction**: Since the equilibrium is shifting to the left at high temperature, we can conclude that the reaction is exothermic. This means that the enthalpy change (\( \Delta H \)) is negative (\( \Delta H < 0 \)). 6. **Conclusion on Moles**: Since the equilibrium is shifting to the left, the number of moles of reactants \( (A + B) \) will be greater than the number of moles of products \( (C + D) \). Thus, we can express this as: \[ a + b > c + d \] 7. **Final Answer**: The correct set of conditions that describe the equilibrium shift is: - \( a + b > c + d \) (more moles of reactants than products) - \( \Delta H < 0 \) (the reaction is exothermic)
To solve the question regarding the equilibrium reaction \( aA + bB \rightleftharpoons cC + dD \) under low pressure and high temperature conditions, we will analyze how these conditions affect the equilibrium position. ### Step-by-step Solution: 1. **Understand the Reaction**: The equilibrium reaction is given as \( aA + bB \rightleftharpoons cC + dD \). Here, \( A \) and \( B \) are the reactants, while \( C \) and \( D \) are the products. 2. **Identify the Conditions**: The question specifies low pressure and high temperature. We need to determine how these conditions affect the equilibrium position. ...
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