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Chapter 17: Q5P (page 775)

White phosphorous, p4, is produced by the reduction of phosphate rock, Ca3(PO4)2.If exposed to oxygen, the waxy, white solid smokes, bursts into flames, and releases a large quantity of heat. Does the reactionP4(g)+5O2(g)𝆏P4O10(S) have a large or small equilibrium constant? Explain.

Short Answer

Expert verified

The answer is,

Yes, a small equilibrium constant

Step by step solution

01

Equilibrium

The equilibrium state of a reaction is represented using the double-headed arrows and the equilibrium constant is used to denote the scene mathematically. It is the ratio of the concentration of products to the ratio of the concentration of the reactants.

02

Explanation

The equilibrium constant K of a reaction is written as the ratio of the concentration of the products to the concentration of the reactants of the aqueous or gaseous substances. The solid and liquid substances are omitted from the equilibrium constant equation.

Hence the equilibrium constant of the given equation can be written as shown below.

K=1P4O25

Therefore the value of K will be very small.

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Most popular questions from this chapter

Gaseous decomposes according to the reaction

PCI5(g)□PCI3(g)+CI2(g)

In one experiment, 0.15 mol of PCI5(g)was introduced into a 2.0-L container.

Construct the reaction table for this process.

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

Le Châtelier's principle is related ultimately to the rates of the forward and reverse steps in a reaction. Explain (a) why an increase in reactant concentration shifts the equilibrium position to the right but does not change K; (b) why a decrease in V shifts the equilibrium position toward fewer moles of gas but does not change K; (c) why a rise in T shifts the equilibrium position of an exothermic reaction toward reactants and also changes K; and (d) why a rise in temperature of an endothermic reaction from T1to T2results in K2 being larger thanK1 .

Balance each reaction and write its reaction quotient, Qc:

(a)C2H6(g)+O2(g)𝆏CO2(g)+H2O(g)(b)CH4(g)+F2(g)𝆏CF4(g)+4HF(g),(c)SO3(g)𝆏SO2(G)+O2(g),

Does Q for the formation of 1 mol of NO from its elements differ from Q for the decomposition of 1 mol of NO to its elements? Explain and give the relationship between the two Q’s.
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