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For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.
Which of the following statements is incorrect?
- a)The equilibrium will shift in forward direction as the pressure increases.
- b)The addition of inert gas at constant volume will not affect the equilibrium constant.
- c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.
- d)The equilibrium constant decreases as the temperature increases.
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC...
Explanation:
To understand why option C is incorrect, let's analyze the given statement and the information provided in the question.
The statement in option C says that "The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required." However, this statement is incorrect because the equilibrium constant does not indicate whether a reaction will go to completion or not. The equilibrium constant only gives information about the position of the equilibrium and the relative concentrations of the reactants and products at equilibrium.
Now, let's analyze each option to understand why the other options are correct:
a) The equilibrium will shift in the forward direction as the pressure increases:
According to Le Chatelier's principle, if the pressure is increased, the equilibrium will shift in the direction that reduces the total number of moles of gas. In this case, the forward reaction has a decrease in the number of moles of gas (2 moles of SO2 + 1 mole of O2 = 2 moles of SO3), so the equilibrium will shift in the forward direction to reduce the pressure. Therefore, option a) is correct.
b) The addition of an inert gas at constant volume will not affect the equilibrium constant:
The equilibrium constant (Kc) is defined as the ratio of the concentrations of the products to the concentrations of the reactants, raised to the power of their stoichiometric coefficients. The addition of an inert gas does not change the concentrations of the reactants or products, so it does not affect the equilibrium constant. Therefore, option b) is correct.
d) The equilibrium constant decreases as the temperature increases:
According to the Van't Hoff equation, the equilibrium constant (Kc) is dependent on the temperature. For an exothermic reaction (where heat is released), an increase in temperature will decrease the equilibrium constant. In this case, since the reaction is exothermic (as indicated by the negative value of enthalpy, H), an increase in temperature will decrease the equilibrium constant. Therefore, option d) is correct.
In conclusion, the incorrect statement is option C) "The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required." The equilibrium constant does not indicate whether a reaction will go to completion or not.
To understand why option C is incorrect, let's analyze the given statement and the information provided in the question.
The statement in option C says that "The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required." However, this statement is incorrect because the equilibrium constant does not indicate whether a reaction will go to completion or not. The equilibrium constant only gives information about the position of the equilibrium and the relative concentrations of the reactants and products at equilibrium.
Now, let's analyze each option to understand why the other options are correct:
a) The equilibrium will shift in the forward direction as the pressure increases:
According to Le Chatelier's principle, if the pressure is increased, the equilibrium will shift in the direction that reduces the total number of moles of gas. In this case, the forward reaction has a decrease in the number of moles of gas (2 moles of SO2 + 1 mole of O2 = 2 moles of SO3), so the equilibrium will shift in the forward direction to reduce the pressure. Therefore, option a) is correct.
b) The addition of an inert gas at constant volume will not affect the equilibrium constant:
The equilibrium constant (Kc) is defined as the ratio of the concentrations of the products to the concentrations of the reactants, raised to the power of their stoichiometric coefficients. The addition of an inert gas does not change the concentrations of the reactants or products, so it does not affect the equilibrium constant. Therefore, option b) is correct.
d) The equilibrium constant decreases as the temperature increases:
According to the Van't Hoff equation, the equilibrium constant (Kc) is dependent on the temperature. For an exothermic reaction (where heat is released), an increase in temperature will decrease the equilibrium constant. In this case, since the reaction is exothermic (as indicated by the negative value of enthalpy, H), an increase in temperature will decrease the equilibrium constant. Therefore, option d) is correct.
In conclusion, the incorrect statement is option C) "The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required." The equilibrium constant does not indicate whether a reaction will go to completion or not.
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Community Answer
For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC...
Explanation:
The incorrect statement is option C: The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.
Reasoning:
To understand why option C is incorrect, we need to consider the concept of equilibrium and the role of a catalyst in a chemical reaction.
Equilibrium:
In a reversible chemical reaction, such as the one given in the question, the reactants can react to form products, and the products can also react to reform the reactants. At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction, resulting in no net change in the concentrations of the reactants and products.
Equilibrium Constant:
The equilibrium constant (Kc) is a measure of the extent to which a chemical reaction proceeds at equilibrium. It is calculated by taking the ratio of the concentrations of the products to the concentrations of the reactants, each raised to their respective stoichiometric coefficients.
In the given reaction, the equilibrium constant (Kc) is 1.7 x 1016, which is a very large value. This indicates that at equilibrium, the concentration of the products (SO3) is much higher compared to the concentration of the reactants (SO2 and O2).
Role of Catalyst:
A catalyst is a substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy. It does not get consumed in the reaction and does not affect the equilibrium position or the equilibrium constant.
Explanation of Incorrect Statement:
Option C states that since the equilibrium constant is large, the reaction goes to completion and no catalyst is required. However, this statement is incorrect for the given reaction because:
1. Equilibrium Constant (Kc): The magnitude of the equilibrium constant does not indicate the extent to which a reaction goes to completion. It only provides information about the relative concentrations of the reactants and products at equilibrium. In this case, a large equilibrium constant suggests that the concentration of the products is favored over the concentration of the reactants at equilibrium, but it does not imply that the reaction goes to completion.
2. Catalyst Requirement: The need for a catalyst in a reaction is determined by the reaction kinetics, which is related to the rate of the reaction. A catalyst can increase the rate of a reaction, but it does not affect the equilibrium position or the equilibrium constant. In this case, the presence or absence of a catalyst is unrelated to the magnitude of the equilibrium constant.
Therefore, option C is incorrect because the equilibrium constant does not determine the need for a catalyst, and a large equilibrium constant does not imply that the reaction goes to completion.
The incorrect statement is option C: The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.
Reasoning:
To understand why option C is incorrect, we need to consider the concept of equilibrium and the role of a catalyst in a chemical reaction.
Equilibrium:
In a reversible chemical reaction, such as the one given in the question, the reactants can react to form products, and the products can also react to reform the reactants. At equilibrium, the rate of the forward reaction is equal to the rate of the backward reaction, resulting in no net change in the concentrations of the reactants and products.
Equilibrium Constant:
The equilibrium constant (Kc) is a measure of the extent to which a chemical reaction proceeds at equilibrium. It is calculated by taking the ratio of the concentrations of the products to the concentrations of the reactants, each raised to their respective stoichiometric coefficients.
In the given reaction, the equilibrium constant (Kc) is 1.7 x 1016, which is a very large value. This indicates that at equilibrium, the concentration of the products (SO3) is much higher compared to the concentration of the reactants (SO2 and O2).
Role of Catalyst:
A catalyst is a substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lower activation energy. It does not get consumed in the reaction and does not affect the equilibrium position or the equilibrium constant.
Explanation of Incorrect Statement:
Option C states that since the equilibrium constant is large, the reaction goes to completion and no catalyst is required. However, this statement is incorrect for the given reaction because:
1. Equilibrium Constant (Kc): The magnitude of the equilibrium constant does not indicate the extent to which a reaction goes to completion. It only provides information about the relative concentrations of the reactants and products at equilibrium. In this case, a large equilibrium constant suggests that the concentration of the products is favored over the concentration of the reactants at equilibrium, but it does not imply that the reaction goes to completion.
2. Catalyst Requirement: The need for a catalyst in a reaction is determined by the reaction kinetics, which is related to the rate of the reaction. A catalyst can increase the rate of a reaction, but it does not affect the equilibrium position or the equilibrium constant. In this case, the presence or absence of a catalyst is unrelated to the magnitude of the equilibrium constant.
Therefore, option C is incorrect because the equilibrium constant does not determine the need for a catalyst, and a large equilibrium constant does not imply that the reaction goes to completion.
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For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer?
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For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer?.
For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer?.
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ample number of questions to practice For the reaction, 2SO2(g) + O2(g) = 2SO3(g), H = -57.2 kJ mol-1 and KC = 1.7 x 1016.Which of the following statements is incorrect?a)The equilibrium will shift in forward direction as the pressure increases.b)The addition of inert gas at constant volume will not affect the equilibrium constant.c)The equilibrium constant is large, which is suggestive of the reaction going to completion, so no catalyst is required.d)The equilibrium constant decreases as the temperature increases.Correct answer is option 'C'. Can you explain this answer? tests, examples and also practice JEE tests.
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