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Chapter 13: Q61 E (page 757)

Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.

Short Answer

Expert verified

a)

2SO3(g) (g)⇌ 2HO2(g)+ O2(g)

Change in concentration

\[ - 2x\]

\[ + 2x\]

\[ + x\]

Change in concentration

\[ - 0.125 \cdot 2 = - 0.250M\]

\[ + 0.125 \cdot 2 = + 0.250M\]

\[ + 0.125{\rm{M}}\]

b)

4NH3(g) + 3O2(g)⇌ 2N2O (g) 6H2 O(g)

Change in concentration

\[ + 4x\]

\[ + 3x\]

\[ - 2x\]

$ + 6x$

Change in concentration

\[\frac{{0.24M}}{3} \cdot 4 = + 0.32M\]

\[ + 0.24{\rm{M}}\]

\[ - \frac{{0.24M}}{3} \cdot 2 = - 0.16M\]

\[ - \frac{{0.24M}}{3} \cdot 6 = - 0.48M\]

c)

2CH4 (g)⇌ C2H2 (g) 3H2(g)

Change in concentration

\[ - 2x\]

\[ + x\]

\[ + 3x\]

Change in concentration

\[ - 25 \cdot 2 = - 50{\rm{\;torr\;}}\]

\[25{\rm{\;torr\;}}\]

\[ + 25{\rm{\;torr\;}} \cdot 3 = + 75{\rm{\;torr\;}}\]

d)

CH4 (g) + H2O(g)⇌ CO(g)

Change in concentration

\[ + x\]

\[ + x\]

\[ - x\]

$ - 3x$

Change in concentration

\[ + 5atm\]

\[5{\rm{atm}}\]

\[ - 5atm\]

\[ - 5{\rm{atm}} \cdot 3 = - 15{\rm{atm}}\]

e)

NH4Cl(s)⇌NH3(g) + HCl (g)

Change in concentration

\[ + x\]

\[ + x\]

Change in concentration

\[1.03 \cdot {10^{ - 4}}{\rm{M}}\]

\[ + 1.03 \cdot {10^{ - 4}}{\rm{M}}\]

f)

Ni (s) + 4CO (g)⇌Ni(CO)4 (g)

Change in concentration

\[ + 4x\]

\[ - x\]

Change in concentration

\[0.40atm\]

\[ - \frac{{0.40{\rm{atm}}}}{4} = - 0.10{\rm{atm}}\]

Step by step solution

01

Definition of change in concentration

The rate of a chemical reaction is defined as the rate of change in concentration of a reactant or product divided by its coefficient from the balanced equation.

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Most popular questions from this chapter

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 \(0.10M\)?

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

\({K_c} = 160\)

Complete the changes in concentrations (or pressure, if requested) for each of the following reactions.

A student solved the following problem and found the equilibrium concentrations to be \(\left[ {S{O_2}} \right] = 0.590M\), \(\left[ {{O_2}} \right] = 0.0450M\), and \(\left[ {S{O_3}} \right] = 0.260M\). How could this student check the work without reworking the problem? The problem was: For the following reaction at \(60{0^0}C\):

\(2S{O_2}(g) + {O_2}(g) \rightleftharpoons 2S{O_3}(g)\)

\({K_c} = 4.32\)

What are the equilibrium concentrations of all species in a mixture that was prepared with \(\left[ {S{O_3}} \right] = 0.500M\), \(\left[ {S{O_2}} \right] = 0M\)and \(\left[ {{O_2}} \right] = 0.350M\)?

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.
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