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Chapter 17: Q17.6P (page 775)

For a given reaction at a given temperature, the value of K is constant. Is the value of Q also constant? Explain.

Short Answer

Expert verified

The answer is,

Yes

Step by step solution

01

Equilibrium constant and reaction quotient

The equilibrium constant can be defined as the ratio of the concentration of products to the ratio of the concentration of the reactants. The equilibrium constant is equal to the reaction quotient when the system is at equilibrium.

02

Explanation

The reaction quotient Q is the ratio of the concentration of the products and the reactants. It is a quantity of relative amount of reactant and products at a given time and at a particular temperature. Hence the reaction quotient is a constant at a particular temperature and is equal to the equilibrium constant at equilibrium.

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Most popular questions from this chapter

Which of the following situations represent equilibrium?

(a) Migratory birds fly north in summer and south in winter.

(b) In a grocery store, some carts are kept inside and some outside. Customers bring carts out to their cars, while store clerks bring carts in to replace those taken out.

(c) In a tug o鈥� war, a ribbon tied to the center of the rope moves back and forth until one side loses, after which the ribbon goes all the way to the winner鈥檚 side.

(d) As a stew is cooking, water in the stew vaporizes, and the vapor condenses on the lid to droplets that drip into the stew.

As an EPA scientist studying catalytic converters and urban smog, you want to find Kcfor the following reaction:

2NO2(g)鈫�N2(g)+2O2(g)Kc=?

Use the following data to find the unknown :

12N2(g)+12O2(g)鈫�NO(g)Kc=4.8脳10-102NO2(g)鈫�2NO(g)+O2(g)Kc=1.1脳10-5

Consider the formation of ammonia in two experiments.

  1. To a 1.00-L container at727oC1.30mol of N2and 1.65molofH2are added. At equilibrium, 0.100molofNH3 is present. Calculate the equilibrium concentrations of N2andH2, and find Kcfor the reaction: 2NH3(g)鈫�N2(g)+3H2(g)
  2. In a different 1.00-L container at the same temperature, equilibrium is established with 8.34脳10-2molofNH3,1.50molofN2,and1.25molofH2 present. CalculateKc for the reaction:NH3(g)鈫�N2(g)+32H2(g)
  3. (c) What is the relationship between the Kc values in parts (a) and (b) ? Why aren't these values the same?

The kinetics and equilibrium of the decomposition of hydrogen iodide have been studied extensively:

2HI(g)鈬�H2(g)+I2(g)

(a) At298K,Kc=1.26脳10-3for this reaction. Calculate Kp.

(b) CalculateKcfor the formation of HIat 298K.

(c)Calculate localid="1657006587824" 螖贬rxnoforlocalid="1657006574683" HIdecomposition from 螖贬fovalues.

(d) At729K,Kc=2.0脳10-2for HIdecomposition. Calculate螖贬rxnfor this reaction from the Vant-Hoff equation.

Use each of the following reaction quotients to write the balanced equation:

(a) Q=[CO2]2[H2O]2[C2H4][O2]3

(b)Q=[NH3]4[O2]7[NO2]4[H2O]6
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