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Chapter 13: Problem 9

The value of the equilibrium constant \(K\) depends on which of the following (more than one answer may be correct)? a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.

Short Answer

Expert verified
The value of the equilibrium constant (K) depends on the temperature of the system (option 'c') and the nature of the reactants and products (option 'd'). It is independent of the initial concentrations of reactants and products (options 'a' and 'b'). Changes in temperature can affect the balance between forward and reverse reaction rates, while the specific chemical properties of reactants and products determine the unique equilibrium constant value for each reaction.

Step by step solution

01

Option a: The initial concentrations of the reactants

The value of the equilibrium constant (K) is independent of the initial concentrations of the reactants. Equilibrium conditions depend on a fixed ratio of the concentrations of reactants and products, irrespective of their initial concentrations. Hence, option 'a' is incorrect.
02

Option b: The initial concentrations of the products

Similar to option 'a', the value of the equilibrium constant (K) is independent of the initial concentrations of the products. The equilibrium concentrations are determined by the fixed ratio between the concentrations of reactants and products, which does not depend on their initial concentrations. So, option 'b' is also incorrect.
03

Option c: The temperature of the system

The value of the equilibrium constant (K) is dependent on the temperature of the system for a given reaction. A change in temperature affects the equilibrium constant because it influences the balance between the forward and reverse reaction rates. If a reaction is endothermic, an increase in temperature will shift the equilibrium to favor the products, increasing the value of K. Conversely, if a reaction is exothermic, an increase in temperature will shift the equilibrium to favor the reactants, decreasing the value of K. Therefore, option 'c' is correct.
04

Option d: The nature of the reactants and products

The value of the equilibrium constant (K) depends on the nature of the reactants and products involved in the reaction. The equilibrium constant represents the balance between the forward and reverse reactions, which in turn depends on the specific chemical properties of the reactants and products. Each reaction has a unique equilibrium constant value that is specific to the reactants and products involved. So, option 'd' is correct. In conclusion, the value of the equilibrium constant (K) depends on the temperature of the system (option 'c') and the nature of the reactants and products (option 'd').

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Most popular questions from this chapter

An important reaction in the commercial production of hydrogen is $$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g)$$ How will this system at equilibrium shift in each of the five following cases? a. Gaseous carbon dioxide is removed. b. Water vapor is added. c. In a rigid reaction container, the pressure is increased by adding helium gas. d. The temperature is increased (the reaction is exothermic). e. The pressure is increased by decreasing the volume of the reaction container.

An 8.00 -g sample of \(\mathrm{SO}_{3}\) was placed in an evacuated container, where it decomposed at \(600^{\circ} \mathrm{C}\) according to the following reaction: $$\mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g)$$ At equilibrium the total pressure and the density of the gaseous mixture were 1.80 \(\mathrm{atm}\) and 1.60 \(\mathrm{g} / \mathrm{L}\) , respectively. Calculate \(K_{\mathrm{p}}\) for this reaction.

Consider the decomposition of the compound \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}\) as follows: $$\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{6}(g)+3 \mathrm{CO}(g)$$ When a 5.63 -g sample of pure \(\mathrm{C}_{5} \mathrm{H}_{6} \mathrm{O}_{3}(g)\) was sealed into an otherwise empty \(2.50-\mathrm{L}\) flask and heated to \(200 .^{\circ} \mathrm{C},\) the pres- sure in the flask gradually rose to 1.63 \(\mathrm{atm}\) and remained at that value. Calculate \(K\) for this reaction.

Solid \(\mathrm{NH}_{4} \mathrm{HS}\) decomposes by the following endothermic process: $$\mathrm{NH}_{4} \mathrm{HS}(s) \leftrightharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{S}(g)$$ a. What effect will adding more \(\mathrm{NH}_{3}(g)\) have on the equilibrium? b. What effect will adding more \(\mathrm{NH}_{4} \mathrm{HS}(s)\) have on the equilibrium? c. What effect will increasing the volume of the container have on the equilibrium? d. What effect will decreasing the temperature have on the equilibrium?

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 \(\mathrm{atm}\) at \(700^{\circ} \mathrm{C} .\)
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