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Chapter 13: Q32 E (page 752)

Explain how to recognize the conditions under which changes in pressure would affect systems at equilibrium.

Short Answer

Expert verified
  • If the number of moles of gas on product side is higher than on reactant side:
    The increase in pressure will shift equilibrium to the left (reactant side)
    The decrease in pressure will shift equilibrium to the right(product side)
  • If the number of moles of gas on reactant side is higher than on product side:
    The increase in pressure will shift equilibrium to the right (product side)
    The decrease in pressure will shift equilibrium to the left(reactant side)
  • If the number of moles of gas on reactant side is equal to the number of moles of gas on product side:
    Therefore, the change in pressure will not have an effect on equilibrium.

Step by step solution

01

Step 1:

Let us explain the conditions under which changes in pressure would affect systems at equilibrium.

  • Le Ch芒telier鈥檚 principle - if a system at equilibrium is disturbed, the equilibrium will shift so as to tend to counteract the effect of the disturbance.
  • The change in pressure will have a effect only on systems with gases and only if there are different numbers of moles of gas on the reactant and product sides of the equilibrium.
  • If the number of moles of gas on product side is higher than on reactant side:
  • The increase in pressure will shift equilibrium to the left (reactant side)
  • The decrease in pressure will shift equilibrium to the right(product side)
  • If the number of moles of gas on reactant side is higher than on product side:
  • The increase in pressure will shift equilibrium to the right (product side)
  • The decrease in pressure will shift equilibrium to the left(reactant side)
  • If the number of moles of gas on reactant side is equal to the number of moles of gas on product side:

The change in pressure will not have an effect on equilibrium.

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Most popular questions from this chapter

Assume that the change in pressure of \({H_2}S\) is small enough to be neglected in the following problem.(a) Calculate the equilibrium pressures of all species in an equilibrium mixture that results from the decomposition of H2S with an initial pressure of 0.824 atm.

\(2{H_2}S(g) \rightleftharpoons 2{H_2}(g) + {S_2}(g)\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,{K_p} = 2.2 \times {10^{( - 6)}}\)

(b) Show that the change is small enough to be neglected.

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.

What is the pressure of \(BrCl\) in an equilibrium mixture of \(C{l_2}\), \(B{r_2}\), and \(BrCl\) if the pressure of \(C{l_2}\) in the mixture is \(0.115atm\)and the pressure of \(B{r_2}\) in the mixture is \(0.450atm\)?

\(C{l_2}(g) + B{r_2}(g) \rightleftharpoons 2BrCl(g)\)

\({K_P} = 4.7 \times 1{0^{ - 2}}\)

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.

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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