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Chapter 17: Q4P (page 775)

Is K very large or very small for a reaction that goes essentially to completion? Explain.

Short Answer

Expert verified

The answer is,

No

Step by step solution

01

Equilibrium

The equilibrium constant is the ratio of the concentration of products to the ratio of the concentration of the reactants. The constant is represented by the letter K.

02

Explanation

The equilibrium constant K does not necessarily be a large value or a small value. But the large value indicates a higher concentration of products. A higher concentration of products gives the completion of a reaction. The small value indicates the higher concentration of the reactants. The reaction can reach the equilibrium condition when it goes to completion.

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Most popular questions from this chapter

Consider the following reaction:

3Fe(s)+4H2O(g)鈬�Fe3O4(s)+4H2(g)

(a) What is the apparent oxidation state ofFe in Fe3O4 ?

(b) Actually, Fe has two oxidation states in Fe3O4. What are they?

(c) At 900掳C,Kcfor the reaction is 5.1. If 0.050molofH2O(g) and 0.100mol ofFe(s) are placed in a1.0鈭�L container at900掳C , how many grams of Fe3O4 are present at equilibrium?

Note: The synthesis of ammonia is a major process throughout the industrialized world. Problems 17.99 to 17.105 refer to various aspects of this all-important reaction:

N2(g)+3H2(g)鈬�2NH3(g)鈥夆赌夆赌�螖贬rxn掳=鈭�91.8kJ

Predict the effect of increasing the container volume on the amounts of each reactant and product in the following reactions:

(a) CH3OH(I)鈬�CH3OH(g)

(b) CH4(g)+NH3(g)鈬�HCN(g)+3H2(g)

Highly toxic disulfurdecafluoride decomposes by a free radical process: S2F10(g)鈬�SF4(g)+SF6(g) . In a study of the decomposition,S2F10 was placed in a2.0 L- flask and heated to100掳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?

The formation of methanol is important to the processing of new fuels. At 298K,KP=2.25脳104for the reaction


localid="1662026070224" CO(g)+2H2(g)鈬�CH3OH(I)

If鈭�Hran=-128kJ/molCH3OH, calculate Kpat 0掳C.

When ammonia is made industrially, the mixture of N2,H2, anddata-custom-editor="chemistry" NH3 that emerges from the reaction chamber is far from equilibrium. Why does the plant supervisor use reaction conditions that produce less than the maximum yield of ammonia?
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