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Chapter 13: Q69E (page 759)

Cobalt metal can be prepared by reducing cobalt (II) oxide with carbon monoxide.

\(CoO(s) + CO(g) \rightleftharpoons Co(s) + C{O_2}(g)\)

\({K_c} = 4.90 \times 1{0^2}at55{0^o}C\)

What concentration of \(CO\) remains in an equilibrium mixture with \(\left[ {C{O_2}} \right] = 0.100M\)

Short Answer

Expert verified

The concentration of CO at equilibrium is \(2.04 \times 1{0^{ - 4}}M\)

Step by step solution

01

Given information

\(CoO(s) + CO(g) \rightleftharpoons Co(s) + C{O_2}(g)\)

  1. Value of equilibrium constant \({K_C} = 4.90 \times 1{0^2}\)
  2. The concentration of \(C{O_2}\) is \(0.100\,M\)

The value of equilibrium molar concentration needs to be calculated using the equation relating equilibrium constant and molar concentrations.

02

Calculate concentration of CO at equilibrium

\(\begin{array}{*{20}{c}}{{K_c}}&{ = \frac{{\left[ {{\rm{C}}{{\rm{O}}_2}} \right]}}{{[{\rm{CO}}]}}}\\{[CO]}&{ = \frac{{\left[ {C{O_2}} \right]}}{{{K_c}}}}\\{}&{ = \frac{{0.100}}{{4.90 \times {{10}^2}}}}\\{}&{ = 2.04 \times {{10}^{ - 4}}{\rm{M}}}\end{array}\)

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Most popular questions from this chapter

Question:Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. \(C{H_4}(g) + {H_2}O(g) \rightleftharpoons 3{H_2}(g) + CO(g)\)

For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%.

Is \({K_c} > 1,\; < 1\), or \( \approx 1\) for a titration reaction?

Which of the systems described in Exercise 13.16 give homogeneous equilibria? Which give heterogeneous equilibria?

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

(b) \(4N{H_3}(g) + 5{O_2}(g)\rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

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

(d) \(C{O_2}(g) + {H_2}(g)\rightleftharpoons CO(g) + {H_2}O(g)\)

(e) \(N{H_4}Cl(s)\rightleftharpoons N{H_3}(g) + HCl(g)\)

(f) \(2\;Pb{\left( {N{O_3}} \right)_2}(s)\rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)

(g) \(2{H_2}(g) + {O_2}(g)\rightleftharpoons 2{H_2}O(l)\)

(h) \({S_8}(g)\rightleftharpoons 8\;S(g)\)

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:

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

Question: The hydrolysis of the sugar sucrose to the sugars glucose and fructose follows a first-order rate equation for the disappearance of sucrose.

C12 H22 O11(aq) + H2O(l)⟶C6 H12 O6 (aq) + C6 H12 O6 (aq)

Rate = k[C12H22O11]

In neutral solution, k = 2.1 × 10−11/s at 27 °C. (As indicated by the rate constant, this is a very slow reaction. In the human body, the rate of this reaction is sped up by a type of catalyst called an enzyme.) (Note: That is not a mistake in the equation—the products of the reaction, glucose and fructose, have the same molecular formulas, C6H12O6, but differ in the arrangement of the atoms in their molecules). The equilibrium constant for the reaction is 1.36 × 105 at 27 °C. What are the concentrations of glucose, fructose, and sucrose after a 0.150 M aqueous solution of sucrose has reached equilibrium? Remember that the activity of a solvent (the effective concentration) is 1.
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