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Chapter 13: Q53E (page 755)

Question:What is the value of the equilibrium constant at \(50{0^o}C\) for the formation of \(N{H_3}\)according to the following equation? N2(g) + 3H2(g) ⇌ 2NH3(g)

An equilibrium mixture of \(N{H_3}(g)\) \({H_2}(g)\) and \({N_2}(g)\) at \(50{0^o}C\) was found to contain\(1.35M{H_2},1.15M{N_2}\)and \(4.12\)\( \times 1{0^{ - 1}}MN{H_3}\)

Short Answer

Expert verified

Theequilibrium constant\({\rm{K}}\{ c\} = 6.00 \times 10\left\{ {^{ - 2}} \right\}\)

Step by step solution

01

Define Equilibrium constant

The Definition of equilibrium constant: a number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a given temperature

02

The mixture of equilibrium constant

Theformation of equation\({\rm{N}}{{\rm{H}}_3}(g)\)\({{\rm{H}}_2}(g)\)\({{\rm{N}}_2}(g)\)

\({\rm{K}}\{ c\} = 6.00 \times 10\left\{ {^{ - 2}} \right\}\)

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Most popular questions from this chapter

Question: The binding of oxygen by hemoglobin (Hb), giving oxyhemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized as

HbO2(aq) + H3 O+(aq) + CO2(g) ⇌ CO2 −Hb−H+ + O2(g) + H2 O(l)

(a) Write the equilibrium constant expression for this reaction.

(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxyhemoglobin in the blood passing through the muscle.

Question: An equilibrium is established according to the following equation

\({K_c} = 4.6\)

What will happen in a solution that is 0.20 M in each \({\rm{Hg}}_2^{2 + },{\rm{NO}}_3^ - ,{{\rm{H}}^ + },{\rm{H}}{{\rm{g}}^{2 + }}\)and \({\rm{HN}}{{\rm{O}}_2}{\rm{\;?\;}}\)

a)\({\rm{H}}{{\rm{g}}_2}^{2 + }\) will be oxidized and \({\rm{N}}{{\rm{O}}_3}\)reduced,

b) \({\rm{H}}{{\rm{g}}_2}^{2 + }\)will be oxidized and \({\rm{N}}{{\rm{O}}_3}\) oxidized.

c)\({\rm{H}}{{\rm{g}}_2}^{2 + }\)will be oxidized and \({\rm{HN}}{{\rm{O}}_2}\)reduced.

d) \({\rm{H}}{{\rm{g}}_2}^{2 + }\)will be oxidized and \({\rm{HN}}{{\rm{O}}_2}\)oxidized.

(e) There will be no change because all reactants and products have an activity of 1.

Question: A reaction is represented by this equation: \({K_c} = 1 \times 1{0^3}\)

(a) Write the mathematical expression for the equilibrium constant.

What would happen to the color of the solution in part (b) if a small amount of \({\bf{NaOH}}\) were added and \({\bf{Fe}}\left( {{\bf{OH}}} \right){\bf{3}}\) precipitated? Explain your answer.

Carbon reacts with water vapor at elevated temperatures

\(C(s) + {H_2}O(g) \rightleftharpoons CO(g) + {H_2}(g)\)

\({K_c} = 0.2at100{0^o}C\)

What is the concentration of CO in an equilibrium mixture with \(\left[ {{H_2}O} \right] = 0.500M\)at \(100{0^0}C\)?
See all solutions

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