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Chapter 12: 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 involved in the reaction (option d). Initial concentrations of reactants and products (options a and b) only affect the position of equilibrium but not the value of K.

Step by step solution

01

Understanding the meaning of the equilibrium constant

The equilibrium constant (K) is a numerical value that expresses the ratio of product concentrations to reactant concentrations when a chemical reaction reaches equilibrium. It quantifies the tendency of a reaction to proceed towards completion at a given temperature.
02

Addressing initial concentrations of reactants and products

The initial concentrations of reactants and products affect the position of equilibrium, not the equilibrium constant. Changes in initial concentrations can cause the reaction to shift towards either the reactants' side or the products' side until a new equilibrium position is established. However, the value of the equilibrium constant (K) for a particular reaction remains constant at a given temperature, regardless of the initial concentrations of reactants and products. Therefore, options a and b are incorrect.
03

Analyzing the effect of temperature on the equilibrium constant

The value of the equilibrium constant (K) depends on the temperature of the system. An increase in temperature can cause the value of K to increase or decrease, depending on whether the reaction is endothermic (where heat is absorbed) or exothermic (where heat is released). For endothermic reactions, an increase in temperature will cause K to increase, whereas for exothermic reactions, an increase in temperature will cause K to decrease. Thus, option c is correct.
04

Assessing the impact of the nature of reactants and products on the equilibrium constant

The equilibrium constant (K) depends on the nature of the reactants and products involved in the chemical reaction. Different reactions involving different substances will have different equilibrium constants because the K value is related to the intrinsic properties of the substances and how they interact. Therefore, the value of K is specific to a given reaction and cannot be applied to another reaction with different reactants and products. Hence, option d is correct.
05

Conclusion

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 involved in the reaction (option d). It does not depend on the initial concentrations of reactants and products (options a and b).

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Most popular questions from this chapter

The gas arsine, AsH_, decomposes as follows:$$2 \mathrm{AsH}_{3}(g) \rightleftharpoons 2 \mathrm{As}(s)+3 \mathrm{H}_{2}(g)$$.In an experiment at a certain temperature, pure \(\mathrm{AsH}_{3}(g)\) was placed in an empty, rigid, sealed flask at a pressure of 392.0 torr.After 48 hours the pressure in the flask was observed to be constant at 488.0 torr. a. Calculate the equilibrium pressure of \(\mathrm{H}_{2}(g)\) b. Calculate \(K_{\mathrm{p}}\) for this reaction.

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction $$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)$$.equilibrium constants \(\mathbf{r}_{\mathbf{p}}\).\(300^{\circ} \mathrm{C}, \quad 4.34 \times 10^{-3}\) \(500^{\circ} \mathrm{C}, \quad 1.45 \times 10^{-5}\) \(600^{\circ} \mathrm{C}, \quad 2.25 \times 10^{-6}\) Is the reaction exothermic or endothermic?

At \(900^{\circ} \mathrm{C}, K_{\mathrm{p}}=1.04\) for the reaction $$\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)$$.At a low temperature, dry ice (solid \(\mathrm{CO}_{2}\) ), calcium oxide, and calcium carbonate are introduced into a 50.0 -L reaction chamber. The temperature is raised to \(900^{\circ} \mathrm{C},\) resulting in the dry ice converting to gaseous \(\mathrm{CO}_{2}\). For the following mixtures, will the initial amount of calcium oxide increase, decrease, or remain the same as the system moves toward equilibrium at \(900^{\circ} \mathrm{C} ?\) a. \(655 \mathrm{g} \mathrm{CaCO}_{3}, 95.0 \mathrm{g} \mathrm{CaO}, P_{\mathrm{CO}_{2}}=2.55 \mathrm{atm}\) b. \(780 \mathrm{g} \mathrm{CaCO}_{3}, 1.00 \mathrm{g} \mathrm{CaO}, P_{\mathrm{CO}_{2}}=1.04 \mathrm{atm}\) c. \(0.14 \mathrm{g} \mathrm{CaCO}_{3}, 5000 \mathrm{g} \mathrm{CaO}, P_{\mathrm{CO}_{2}}=1.04 \mathrm{atm}\) d. \(715 \mathrm{g} \mathrm{CaCO}_{3}, 813 \mathrm{g} \mathrm{CaO}, P_{\mathrm{CO}_{2}}=0.211 \mathrm{atm}\)

Methanol, a common laboratory solvent, poses a threat of blindness or death if consumed in sufficient amounts. Once in the body, the substance is oxidized to produce formaldehyde (embalming fluid) and eventually formic acid. Both of these substances are also toxic in varying levels. The equilibrium between methanol and formaldehyde can be described as follows: $$\mathrm{CH}_{3} \mathrm{OH}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}(aq)+\mathrm{H}_{2}(a q)$$. =Assuming the value of \(K\) for this reaction is \(3.7 \times 10^{-10},\) what are the equilibrium concentrations of each species if you start with a \(1.24 M\) solution of methanol? What will happen to the concentration of methanol as the formaldehyde is further converted to formic acid?

Which of the following statements is(are) true? Correct the false statement(s). a. When a reactant is added to a system at equilibrium at a given temperature, the reaction will shift right to reestablish equilibrium. b. When a product is added to a system at equilibrium at a given temperature, the value of \(K\) for the reaction will increase when equilibrium is reestablished. c. When temperature is increased for a reaction at equilibrium, the value of \(K\) for the reaction will increase. d. When the volume of a reaction container is increased for a system at equilibrium at a given temperature, the reaction will shift left to reestablish equilibrium. e. Addition of a catalyst (a substance that increases the speed of the reaction) has no effect on the equilibrium position.
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