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Chapter 5: Problem 164

When two reactants \(\mathrm{A}\) and \(\mathrm{B}\) are mixed to give products \(\mathrm{C}\) and \(\mathrm{D}\), the reaction quotient, \(\mathrm{Q}\), at the initial stages of the reaction a. is zero b. decreases with time c. is independent of time d. increases with time.

Short Answer

Expert verified
d. Increases with time.

Step by step solution

01

Understand the Reaction Quotient, Q

The reaction quotient, \( Q \), is given by the formula \( Q = \frac{[C][D]}{[A][B]} \), where \([C]\), \([D]\), \([A]\), and \([B]\) represent the concentrations of the respective species in the reaction mixture at a given time. At the initial stage of a reaction, \([C]\) and \([D]\) are typically at their lowest, often zero if the reaction has just started, which influences \( Q \).
02

Initial Stage of the Reaction

At the very beginning of the reaction, the concentrations of the products \( C \) and \( D \) are zero, meaning \( [C] = 0 \) and \( [D] = 0 \). Consequently, the reaction quotient \( Q \) is \( Q = \frac{0 \times 0}{[A][B]} = 0 \).
03

Impact of Reaction Progress on Q

As the reaction progresses, \([C]\) and \([D]\) start to form, and their concentrations increase. This results in an increase in the value of \( Q \) over time until the reaction reaches equilibrium.
04

Conclusion about Q

Based on the calculations and understanding from the previous steps, at the initial stages of the reaction, \( Q \) starts at 0 and increases over time as more products are formed and \([C]\) and \([D]\) increase in concentration.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Initial Reaction Stage
When a chemical reaction begins, it is known as the initial reaction stage. At this point, the reactants A and B are present in their original concentrations, and the products C and D have not formed yet.
This is an important time because the reaction quotient, denoted as \( Q \), can be determined.
Initially, the concentrations of C and D are zero because no products have been formed. As a result, the calculation \( Q = \frac{[C][D]}{[A][B]} \) results in a quotient of zero, since \([C]\) and \([D]\) are both zero at the start.
This starting value of zero provides a baseline to observe how the reaction progresses.
  • The initial concentration of products is zero.
  • The reaction quotient \( Q \) starts at zero.
  • This stage sets the groundwork for observing changes as the reaction moves forward.
Concentration Changes
As the chemical reaction advances, the concentrations of products C and D begin to rise while the concentrations of reactants A and B decrease.
This is because reactants are being converted into products.
These changes in concentration are measurable at different time points.
Tracking these changes helps us understand the dynamics of the reaction and how the reaction quotient \( Q \) evolves.
Since \( Q = \frac{[C][D]}{[A][B]} \) depends on the concentration of both products and reactants, the increasing concentration of products leads to an increase in \( Q \) over time.
  • Product concentrations increase as the reaction proceeds.
  • Reactant concentrations decrease parallelly.
  • These changes in concentrations result in an increase in the value of \( Q \).
Equilibrium in Reactions
Reaching equilibrium is an essential aspect of any chemical reaction. At equilibrium, the reactions move forward and backward at the same rate, so concentrations of reactants and products remain constant.
This balance means that the reaction quotient \( Q \) becomes equal to the equilibrium constant \( K \).
The path from the initial reaction to equilibrium shows growing concentrations of products, reducing the concentrations of reactants until the two processes happen simultaneously at equilibrium.
At this point, even though the reaction is still happening, there is no net change in concentrations, so \( Q \) remains constant at \( K \).
  • The reaction reaches a state of balance at equilibrium.
  • \( Q \) matches the equilibrium constant \( K \).
  • Concentration changes stop at equilibrium, maintaining steady values.

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Most popular questions from this chapter

(A): The value of \(\mathrm{K}\) gives us a relative idea about the extent to which a reaction proceeds. \((\mathbf{R}):\) The value of \(\mathrm{K}\) is independent of the stoichiometry of reactants and products at the point of equilibrium.

For the gas phase reaction, \(\mathrm{C}_{2} \mathrm{H}_{4}+\mathrm{H}_{2} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(\Delta \mathrm{H}=-32.7 \mathrm{kcal})\), carried out in a closed vessel, the equilibrium concentration of \(\mathrm{C}_{2} \mathrm{H}_{4}\) can be increased by a. Decreasing the pressure b. Adding some \(\mathrm{C}_{2} \mathrm{H}_{6}\) c. Increasing the temperature d. Removing some \(\mathrm{H}\),

Which of the following is/are correct? a. The equilibrium constant does not depend upon pressure b. When pressure is applied on ice \(\rightleftharpoons\) water equilibrium more water will be formed c. The equilibrium constant increases when a catalyst is introduced d. Changes with temperature

Find the pH of \(0.012 \mathrm{M}\) solution of \(\mathrm{NH}_{4} \mathrm{CN}\) if \(\mathrm{K}_{\mathrm{a}}\) for \(\mathrm{HCN}\) and \(\mathrm{K}_{\mathrm{b}}\) for \(\mathrm{NH}_{3}\) are \(6.2 \times 10^{-10}\) and \(1.6 \mathrm{x}\) \(10^{-5}\) respectively a. \(8.2\) b. \(9.2\) c. \(4.8\) d. \(5.8\)

Consider the following reversible reaction: \(\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})\) \(\Delta \mathrm{H}=-92.5 \mathrm{~kJ}\)Which factor(s) will increase the yield of methanol at equilibrium? a. Addition of inert gas at constant volume b. Increased pressure on the system c. Increased temperature d. Increased partial pressure of hydrogen
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