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Chapter 13: Q28E (page 752)

Write the expression of the reaction quotient for the ionization of HOCN in water.

Short Answer

Expert verified

Therefore,the reaction quotient for the ionization of HOCN in water.

\({Q_c} = \frac{{c\left( {{H_3}{O^ + }} \right) \cdot c\left( {OC{N^ - }} \right)}}{{c(HOCN)}}\).

Step by step solution

01

Reaction regarding ionization of HOCN in water:

First, we will write reaction of dissociation:

\(HOCN(aq) + {H_2}O(l) \to {H_3}{O^ + }(aq) + OC{N^ - }(aq)\)

(Note, there needs to be double arrow, because this is a reverse reaction).

Equation for reaction quotient is the same as for equilibrium constant, but we don't use equilibrium concentrations, but concentrations in any time before equilibrium.

02

The Expression for the reaction quotient for the ionization of HOCN in water:

\({Q_c} = \frac{{c\left( {{H_3}{O^ + }} \right) \cdot c\left( {OC{N^ - }} \right)}}{{c(HOCN)}}\)

Note - water is not included into the equation because it is liquid and its activity is 1 , so it would be like this:

\({Q_c} = \frac{{c\left( {{H_3}{O^ + }} \right) \cdot c\left( {OC{N^ - }} \right)}}{{c(HOCN) \cdot 1}}\).

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Most popular questions from this chapter

Question:Calculate the value of the equilibrium constant \({K_P}\) for the reaction \(2NO(g) + C{l_2}(g) \rightleftharpoons 2NOCl(g)\) from these equilibrium pressures: NO, \(0.050atm;C{l_2},0.30atm;NOCl,1.2atm\)

Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas.

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

\(F{e_2}{O_3}(s) + 3{H_2}(g) \rightleftharpoons 2Fe(s) + 3{H_2}O(g)\) \(\Delta H = 98.7kJ\)

(b) What will happen to the concentration of each reactant and product at equilibrium if more \(Fe\)is added?

(c) What will happen to the concentration of each reactant and product at equilibrium if \({H_2}O\) is removed?

(d) What will happen to the concentration of each reactant and product at equilibrium if \({H_2}\) is added?

(e) What will happen to the concentration of each reactant and product at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

Why are there no changes specified for NH4HS? What property of Ni does change?

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 \(\left[ {C{O_2}} \right] = 0.100M\)

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

\((a)\,C{l_2}\left( g \right) + B{r_2}\left( g \right)\rightleftharpoons 2BrCl(g)\,\,\,{K_C} = 4.7 \times {10^{ - 2}}\,at\,25^\circ C\)

\((b)2{\rm{S}}{{\rm{O}}_2}(g) + {{\rm{O}}_2}(g)\rightleftharpoons 2{\rm{S}}{{\rm{O}}_3}(g){K_P} = 48.2 at {500^\circ} {\rm{C}}\)

\((c){\rm{CaC}}{{\rm{l}}_2} \cdot 6{{\rm{H}}_2}{\rm{O}}(s)\rightleftharpoons {\rm{CaC}}{{\rm{l}}_2}(s) + 6{{\rm{H}}_2}{\rm{O}}(g){K_P} = 5.09 \times {10^{ - 44}}at{25^\circ }{\rm{C}}\)

\((d){{\rm{H}}_2}{\rm{O}}(l)\rightleftharpoons {{\rm{H}}_2}{\rm{O}}(g)\,{K_P} = 0.196\,at\,{60^\circ }{\rm{C}}\)
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