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Chapter 13: Q95E (page 762)

Question: Consider the equilibrium

4NO2(g) + 6H2 O(g) 鈬� 4NH3(g) + 7O2(g)

(a) What is the expression for the equilibrium constant (Kc) of the reaction?

(b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant?

(c) If the reaction were at equilibrium, how would a decrease in pressure (from an increase in the volume of the reaction vessel) affect the pressure of NO2?

(d) If the change in the pressure of NO2 is 28 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of O2 change?

Short Answer

Expert verified
  1. The Expression for the equilibrium constant \({K_c} = \frac{{{{\left( {{\rm{N}}{{\rm{H}}_3}} \right)}^4} \times {{\left( {{{\rm{O}}_2}} \right)}^7}}}{{{{\left( {{\rm{N}}{{\rm{O}}_2}} \right)}^4} \times {{\left( {{{\rm{H}}_2}{\rm{O}}} \right)}^6}}}\)
  2. If the reaction quotient is less than the equilibrium constant\(\left( {Q < {K_c}} \right)\)the reaction will move to the right, therefore the concentration of the\({\rm{N}}{{\rm{H}}_3}\)will increases
  3. The decrease in pressure will move equilibrium to the right (since there are more gas molecules) Therefore, the pressure of\({\rm{N}}{{\rm{O}}_2}\)will decrease.
  4. The Change in pressure of \({{\rm{O}}_2}{\rm{\;will be\;}}49{\rm{\;torr\;}}\)

Step by step solution

01

Definition

Chemical equilibrium is defined as a dynamic state where the concentration of all reactants remains constant. In a chemical reaction, an equilibrium situation is indicated by a double arrow.

02

Expression for the equilibrium constant

\(4{\text{N}}{{\text{O}}_2}({\text{g}}) + 6{{\text{H}}_2}{\text{O}}({\text{g}}) \rightleftharpoons 4{\text{N}}{{\text{H}}_3}({\text{g}}) + 7{{\text{O}}_2}({\text{g}})\)

The equilibrium constant is

\({K_c} = \frac{{{{\left( {N{H_3}} \right)}^4} \times {{\left( {{O_2}} \right)}^7}}}{{{{\left( {N{O_2}} \right)}^4} \times {{\left( {{H_2}O} \right]}^6}}}\)

03

Reaction quotient of the reaction

If the reaction quotient is less than the equilibrium constant \(\left( {Q < {K_c}} \right)\)the reaction will move to the right, therefore the concentration of the \(N{H_3}\)will increases

04

Pressure of the reaction

The decrease in pressure will move equilibrium to the right (since there are more gas molecules) Therefore, the pressure of \(N{O_2}\)will decrease.

05

Change of pressure

\(N{O_2}{\rm{\;\;}}\)is\(28\,torr\)

We have to find how much will the change of pressure of\({O_2}\)be

Four moles of\(N{O_2}\)will produce 7 moles of \({O_2}\). Therefore, If the change in pressure \(N{O_2}{\rm{\;\;}}\)is\(28\,torr\),The change of pressure of\({O_2}\)will be

\({\rm{\;Change\;}}{{\rm{O}}_2}\left( {torr} \right) = 28torr\left( {{\rm{N}}{{\rm{O}}_2}} \right) \times \frac{{7{{\rm{O}}_2}}}{{4{\rm{N}}{{\rm{O}}_2}}} = 49torr\left( {{{\rm{O}}_2}} \right)\)

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Most popular questions from this chapter

Question:The amino acid alanine has two isomers, \(\alpha - alanine\;\)and \(\beta - alanine\;\). When equal masses of these two compounds are dissolved in equal amounts of a solvent, the solution of \(\alpha - alanine\;\)freezes at the lowest temperature. Which form, \(\alpha - alanine\;\)or\(\beta - alanine\;\) has the larger equilibrium constant for ionization \(\left( {HX \rightleftharpoons {H^ + } + {X^ - }} \right)?\)

When heated, iodine vapor dissociates according to this equation: I2 (g) 鈬� 2I (g). At 1274K a sample exhibits a partial pressure of I2 of 0.1122 and a partial pressure due to I atoms of 0.1378 atm. Determine the value of the equilibrium constant, Kp for the decomposition at 1274K

Calculate the pressures of all species at equilibrium in a mixture of NOCl, NO, and Cl2produced when a sample of NOCl with a pressure of 10.0 atm comes to equilibrium according to this reaction:

\(2NOCl(g) \rightleftharpoons 2NO(g) + C{l_2}(g)\quad {K_P} = 4.0 \times 1{0^{ - 4}}\)

Convert the values of Kc to values of Kp or the values of Kp to values of Kc .

\((a)\,{N_2}\left( g \right) + 3{H_2}\left( g \right)\rightleftharpoons 2N{H_3}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_C} = 0.50\,\,at\,\,400^\circ C\)

\((b){{\rm{H}}_2}(g) + {{\rm{I}}_2}(g)\rightleftharpoons 2HI(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_c} = 50.2\,at\,{448^\circ }{\rm{C}}\)

\((c)N{a_2}{\rm{S}}{{\rm{O}}_4} \cdot 10{{\rm{H}}_2}O(s)\rightleftharpoons N{a_2}{\rm{S}}{{\rm{O}}_4}(s) + 10{{\rm{H}}_2}O(g){K_P} = 4.08 \times {10^{ - 25}}at\,{25^\circ }{\rm{C}}\)

\((d){{\rm{H}}_2}{\rm{O}}(l)\rightleftharpoons {{\rm{H}}_2}{\rm{O}}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_P} = 0.122\,at\,{50^\circ }{\rm{C}}\)

Question: In a 3.0-L vessel, the following equilibrium partial pressures are measured: \({{\rm{N}}_2}\),190 torr;\({{\rm{H}}_2}\), 317 torr;\({\rm{N}}{{\rm{H}}_3}\)\(1.00 \times {10^3}\)torr.

  1. How will the partial pressures of\({{\rm{H}}_2},{{\rm{N}}_2}\)and \({\rm{N}}{{\rm{H}}_3}\)change if \({{\rm{H}}_2}\) is removed from the system? Will they increase, decrease, or remain the same?
  2. Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.
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