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When two reactants, A and B are mixed to give products, C and D, the reaction quotient, (Q) at the initial stages of the reaction:
- a)Is zero
- b)Decreases with time
- c)Is independent of time
- d)Increases with time
Correct answer is option 'D'. Can you explain this answer?
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Most Upvoted Answer
When two reactants, A and B are mixed to give products, C and D, the r...
The reaction quotient (Q) and its relation to reactants and products
The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at any given point in time. It is calculated in the same way as the equilibrium constant (K), but it is determined using the concentrations of reactants and products at any moment during the reaction, rather than at equilibrium.
Initial stages of the reaction
In the initial stages of a reaction, before equilibrium is reached, the concentrations of reactants are typically higher compared to the concentrations of products. This is because the reaction has just started, and the products have not had enough time to form in significant amounts. As a result, the value of Q in the initial stages of the reaction is generally smaller than the equilibrium constant, K.
Understanding the options
a) Is zero: This option is incorrect because it implies that no products are formed at the initial stages of the reaction, which is not true. Some products will be present, although in smaller amounts compared to the reactants.
b) Decreases with time: This option is also incorrect because the value of Q does not necessarily decrease with time. It depends on the specific reaction and the rate at which reactants are converted to products.
c) Is independent of time: This option is incorrect because Q changes with time as the reaction progresses. Initially, Q will be smaller than K, but as the reaction proceeds, Q will approach the value of K.
d) Increases with time: This option is the correct answer. As the reaction progresses, reactants are consumed, and products are formed. This leads to an increase in the concentrations of products and a decrease in the concentrations of reactants. Consequently, the value of Q increases with time and approaches the value of K as equilibrium is approached.
Conclusion
In summary, the reaction quotient (Q) at the initial stages of a reaction is smaller than the equilibrium constant (K). As the reaction progresses, Q increases with time and approaches the value of K. The correct answer to the given question is option 'D'.
The reaction quotient (Q) is a measure of the relative concentrations of reactants and products in a chemical reaction at any given point in time. It is calculated in the same way as the equilibrium constant (K), but it is determined using the concentrations of reactants and products at any moment during the reaction, rather than at equilibrium.
Initial stages of the reaction
In the initial stages of a reaction, before equilibrium is reached, the concentrations of reactants are typically higher compared to the concentrations of products. This is because the reaction has just started, and the products have not had enough time to form in significant amounts. As a result, the value of Q in the initial stages of the reaction is generally smaller than the equilibrium constant, K.
Understanding the options
a) Is zero: This option is incorrect because it implies that no products are formed at the initial stages of the reaction, which is not true. Some products will be present, although in smaller amounts compared to the reactants.
b) Decreases with time: This option is also incorrect because the value of Q does not necessarily decrease with time. It depends on the specific reaction and the rate at which reactants are converted to products.
c) Is independent of time: This option is incorrect because Q changes with time as the reaction progresses. Initially, Q will be smaller than K, but as the reaction proceeds, Q will approach the value of K.
d) Increases with time: This option is the correct answer. As the reaction progresses, reactants are consumed, and products are formed. This leads to an increase in the concentrations of products and a decrease in the concentrations of reactants. Consequently, the value of Q increases with time and approaches the value of K as equilibrium is approached.
Conclusion
In summary, the reaction quotient (Q) at the initial stages of a reaction is smaller than the equilibrium constant (K). As the reaction progresses, Q increases with time and approaches the value of K. The correct answer to the given question is option 'D'.
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When two reactants, A and B are mixed to give products, C and D, the r...
Given reaction is A+B⇌C+D
The reaction quotient Q is written by multiplying concentrations of products and dividing by concentration products of reactants
The reaction quotient Q is written by multiplying concentrations of products and dividing by concentration products of reactants
Q = [C][D]/[A][B]
At initial stages of reaction, formation of products C and D takes place; i.e, the concentration od C & D increases at the expenses of A & B concentration, which decreases.
∴Q increases with respect to time
∴Q increases with respect to time
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When two reactants, A and B are mixed to give products, C and D, the reaction quotient, (Q) at the initial stages of the reaction:a)Is zerob)Decreases with timec)Is independent of timed)Increases with timeCorrect answer is option 'D'. Can you explain this answer?
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