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Chapter 17: Q17.9P (page 775)

Explain the difference between a heterogeneous and a homogeneous equilibrium. Give an example of each.

Short Answer

Expert verified

The answer is,

The homogeneous equilibrium is the equilibrium condition in which all the species in the chemical reaction are in the same phase. The heterogeneous equilibrium is the equilibrium condition in which all the species in the chemical reaction are in different phases.

Step by step solution

01

Equilibrium

The equilibrium is the state in which the concentration of reactants and products in a chemical reaction equation is at equilibrium with each other. The equilibrium reactions are written using double-sided arrows.

02

Explanation

The homogeneous equilibrium is the equilibrium condition in which all the species in the chemical reaction are in the same phase. The heterogeneous equilibrium is the equilibrium condition in which all the species in the chemical reaction are in different phases.

Examples of homogeneous reactions are gas-phase reactions or solution reactions.

Examples of heterogeneous equilibrium reactions are the reactions involving the solid and gas phases or solids and liquids.

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Most popular questions from this chapter

Phosgene (COCl2)is a toxic substance that forms readily from carbon monoxide and chlorine at elevated temperatures:

CO(g)+Cl2(g)⇌COCl2(g)

If0.350molof each reactant is placed in a0.500-Lflask at600K, what are the concentrations of all three substances at equilibrium (Kc=4.95at this temperature)?

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)→N2(g)+3H2(g)
  2. In a different 1.00-L container at the same temperature, equilibrium is established with 8.34×10-2molofNH3,1.50molofN2,and1.25molofH2 present. CalculateKc for the reaction:NH3(g)→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?

At 4250C,Kp=4.18×10-9for the reaction

role="math" localid="1655096121156" 2HBr(g)⇌H2(g)+Br2(g)

In one experiment, 0.20 atm of HBr(g), 0.010 atm ofH2(g) , and 0.010 atm ofBr2(g) are introduced into a container. Is the reaction at equilibrium? If not, in which direction will it proceed?

At 100∘C,Kp=60.6for the reaction

2NOBr(g)□2NO(g)+Br2(g)

In a given experiment, 0.10 atm of each component is placed in a container. Is the system at equilibrium? If not, in which direction will the reaction proceed?

Highly toxic disulfurdecafluoride decomposes by a free radical process: S2F10(g)⇌SF4(g)+SF6(g) . In a study of the decomposition,S2F10 was placed in a2.0 L- flask and heated to100°C;[S2F10] was0.50M at equilibrium. MoreS2F10 was added, and when equilibrium was retained,[S2F10] was2.5M . How diddata-custom-editor="chemistry" [SF4]and[SF6] change from the original to the new equilibrium position after the addition of more data-custom-editor="chemistry" S2F10?
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