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Chapter 12: Problem 13

Suppose a reaction has the equilibrium constant \(K=1.3 \times 10^{8} .\) What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?

Short Answer

Expert verified
The equilibrium constant (K) for the reaction is 1.3 × 10^8, which is significantly greater than 1. As a result, the reaction will proceed towards the products and favor the formation of products over reactants at equilibrium. Since the reaction is highly favorable for the formation of products, it is likely to be a good source of the products.

Step by step solution

01

Understanding the Equilibrium Constant

The equilibrium constant, K, is a ratio that compares the concentrations of products and reactants at equilibrium. It is defined as: \( K = \frac{[products]}{[reactants]} \) where [products] and [reactants] represent the concentrations of products and reactants at equilibrium. The value of K indicates the extent to which a reaction will proceed: - If K > 1, the reaction will proceed towards the products (favoring products). - If K = 1, the reaction is balanced between both products and reactants at equilibrium. - If K < 1, the reaction will proceed towards the reactants (favoring reactants).
02

Analyzing the Magnitude of K

For this problem, we are given the equilibrium constant, K = 1.3 × 10^8: - Since K = 1.3 × 10^8, we can identify that K > 1. Therefore, the reaction will proceed towards the products and will favor the formation of products over reactants at equilibrium.
03

Determining the Suitability of the Reaction as a Product Source

Since the equilibrium constant (K = 1.3 × 10^8) is significantly greater than 1, this tells us that the reaction is highly favorable for the formation of products, with a high concentration of products compared to reactants once equilibrium is reached. Based on this information, we can say that the reaction is likely to be a good source of the products.

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Most popular questions from this chapter

At a particular temperature, \(K=3.75\) for the reaction $$\mathrm{SO}_{2}(g)+\mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{SO}_{3}(g)+\mathrm{NO}(g)$$.If all four gases had initial concentrations of 0.800 \(M,\) calculate the equilibrium concentrations of the gases.

Nitrogen gas \(\left(\mathrm{N}_{2}\right)\) reacts with hydrogen gas \(\left(\mathrm{H}_{2}\right)\) to form ammonia \(\left(\mathrm{NH}_{3}\right) .\) At \(200^{\circ} \mathrm{C}\) in a closed container, 1.00 atm of nitrogen gas is mixed with 2.00 atm of hydrogen gas. At equilibrium,the total pressure is 2.00 atm. Calculate the partial pressure of hydrogen gas at equilibrium, and calculate the \(K_{\mathrm{p}}\) value for this reaction.

The equilibrium constant is 0.0900 at \(25^{\circ} \mathrm{C}\) for the reaction $$ \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{Cl}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{HOCl}(g)$$.For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift? a. A 1.0 -L flask contains 1.0 mole of HOCI, 0.10 mole of \(\mathrm{Cl}_{2} \mathrm{O},\) and 0.10 mole of \(\mathrm{H}_{2} \mathrm{O}\) b. A \(2.0-\) L flask contains 0.084 mole of HOCI, 0.080 mole of \(\mathrm{Cl}_{2} \mathrm{O},\) and 0.98 mole of \(\mathrm{H}_{2} \mathrm{O}\) c. A 3.0 -L flask contains 0.25 mole of HOCI, 0.0010 mole of \(\mathrm{Cl}_{2} \mathrm{O},\) and 0.56 mole of \(\mathrm{H}_{2} \mathrm{O}\).

The following equilibrium pressures at a certain temperature were observed for the reaction $$\begin{aligned}2 \mathrm{NO}_{2}(g) & \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \\\P_{\mathrm{NO}_{2}} &=0.55 \mathrm{atm} \\\P_{\mathrm{NO}} &=6.5 \times 10^{-5} \mathrm{atm} \\\P_{\mathrm{O}_{2}} &=4.5 \times 10^{-5} \mathrm{atm}\end{aligned}$$. Calculate the value for the equilibrium constant \(K_{\mathrm{p}}\) at this temperature.

The equilibrium constant \(K_{\mathrm{p}}\) for the reaction $$\mathrm{CCl}_{4}(g) \rightleftharpoons \mathrm{C}(s)+2 \mathrm{Cl}_{2}(g)$$ at \(700^{\circ} \mathrm{C}\) is \(0.76 .\) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at \(700^{\circ} \mathrm{C}\).
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