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Chapter 13: Q56E (page 756)

Question:At 1 atm and \(2{5^o}C,N{O_2}\) with an initial concentration of \(1.00M\;is\;3.3 \times 1{0^{ - 3}}\% \)decomposed into \(NO\;and\;{O_2}\). Calculate the value of the equilibrium constant for the reaction. \(2N{O_2}(g) \rightleftharpoons 2NO(g) + {O_2}(g)\)

Short Answer

Expert verified

The value of \({K_c} = 1.80 \cdot {10^{ - 14}}\)

Step by step solution

01

Define Decomposed

Decomposition or rot is the process by which dead organic substances are broken down into simpler organic or inorganic matter such as carbon dioxide, water, simple sugars and mineral salts

02

Decomposition Reaction

\(2N{O_2}(g) \rightleftharpoons 2NO(g) + {O_2}(g)\)

Calculate the change in concentration of\({\rm{N}}{{\rm{O}}_2}\)

\(\begin{array}{*{20}{c}}{\left( {{\rm{N}}{{\rm{O}}_2}} \right) - \left( {{\rm{N}}{{\rm{O}}_2}} \right)(eq) = \left( {{\rm{N}}{{\rm{O}}_2}} \right) \cdot 3.3 \cdot {{10}^{ - 3}}{\rm{\% }}}\\{ = 1.00{\rm{M}} \cdot 3.3 \cdot {{10}^{ - 3}}{\rm{\% }}}\\{ = 3.3 \cdot {{10}^{ - 5}}{\rm{M}}}\end{array}\)

03

Calculating equilibrium constant

The equilibrium constant for given reaction is

\(\begin{array}{*{20}{c}}{{K_c} = \frac{{{{(NO)}^2} \cdot \left( {{{\rm{O}}_2}} \right)}}{{{{\left( {{\rm{N}}{{\rm{O}}_2}} \right)}^2}}}}\\{ = \frac{{{{\left( {3.3 \cdot {{10}^{ - 5}}} \right)}^2} \cdot \left( {\frac{{3.3 \cdot {{10}^{ - 5}}}}{2}} \right)}}{{{{\left( {1.00 - 3.3 \cdot {{10}^{ - 5}}} \right)}^2}}}}\\{}\end{array}\)

The value of \({K_c} = 1.80 \cdot {10^{ - 14}}\)

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Most popular questions from this chapter

Nitrogen and oxygen react at high temperatures.

(a) Write the expression for the equilibrium constant \(\left( {{K_c}} \right)\)for the reversible reaction

\(\Delta H = 181kJ\)

(b) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if more \({O_2}\)is added?

(c) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if \({N_2}\)is removed?

(d) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if \(NO\)is added?

(e) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if the temperature of the system is increased?

(g) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if a catalyst is added?

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) 鈬� 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 \(4.12\)\( \times 1{0^{ - 1}}MN{H_3}\)

Question: \(\;A\;0.72 - mol\)sample of \(PC{l_5}\)is put into a \(1.00 - L\) vessel and heated. At equilibrium, the vessel contains \(0.40mol\) of \(PC{l_3}(g)\) and \(0.40mol\;of\;C{l_2}(g)\). Calculate the value of the equilibrium constant for the decomposition of \(PC{l_5}\;to\;\)\(PC{l_3}\;and\;C{l_2}\)at this temperature.

Analysis of the gases in a sealed reaction vessel containing \(N{H_3}\), \({N_2}\), and \({H_2}\) at equilibrium at \(40{0^0}C\) established the concentration of \({N_2}\) to be \(1.2M\) and the concentration of \({H_2}\) to be \(0.24M\).

\({N_2}(g) + 3{H_2}(g) \rightleftharpoons 2N{H_3}(g)\)

\({K_c} = 0.50\,at\,40{0^o}C\)

Calculate the equilibrium molar concentration of \(N{H_3}\).

A student solved the following problem and found \(\left[ {{N_2}{O_4}} \right] = 0.16M\)at equilibrium. How could this student recognize that the answer was wrong without reworking the problem? The problem was: What is the equilibrium concentration of \(\left[ {{N_2}{O_4}} \right]\) in a mixture formed from a sample of \(N{O_2}\) with a concentration of \(0.10M\)?

\(2N{O_2}(g) \rightleftharpoons {N_2}{O_4}(g)\)

\({K_c} = 160\)
See all solutions

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