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Chapter 15: Problem 5

Write an equilibrium constant, \(K_{c},\) for the formation from its gaseous elements of \((a) 1\) mol \(\mathrm{HF}(\mathrm{g})\) (b) \(2 \mathrm{mol} \mathrm{NH}_{3}(\mathrm{g}) ;(\mathrm{c}) 2 \mathrm{mol} \mathrm{N}_{2} \mathrm{O}(\mathrm{g}) ;(\mathrm{d}) 1 \mathrm{mol} \mathrm{ClF}_{3}(1)\)

Short Answer

Expert verified
The equilibrium constants are as follows: (a) \(K_{c} = \frac{[HF]^2}{[H_2][F_2]}\) (b) \(K_{c} = \frac{[NH_3]^2}{[N_2][H_2]^3}\) (c) \(K_{c} = \frac{[N_{2O}]^2}{[N_2][O_2]}\) (d) \( K_{c} = \frac{[ClF_{3}]^2}{[Cl_{2}][F_{2}]^3}\)

Step by step solution

01

Write equation for formation of HF(g)

The formation reaction for hydrofluoric acid, \(HF(g)\), can be written as:\[ H_{2(g)} + F_{2(g)} \rightarrow 2HF_{(g)}\]
02

Establish the equilibrium constant expression for HF(g)

The equilibrium constant expression for \(HF(g)\) is the product of the concentrations of the products divided by the product of the concentrations of the reactants, each raised to the power of its stoichiometric coefficient, as follows:\[K_{c} = \frac{[HF]^2}{[H_2][F_2]}\]
03

Write equation for formation of NH3(g)

The formation reaction for ammonia, \(NH_{3(g)}\), is:\[N_{2(g)} + 3H_{2(g)} \rightarrow 2NH_{3(g)}\]
04

Establish the equilibrium constant expression for NH3(g)

The equilibrium constant for this reaction is:\[K_{c} = \frac{[NH_3]^2}{[N_2][H_2]^3}\]
05

Write equation for the formation of N2O(g)

The formation reaction for nitrous oxide, \(N_{2O(g)}\), is:\[N_2(g) + O_2(g) \rightarrow 2N_{2O(g)}\]
06

Establish the equilibrium constant expression for N2O(g)

The equilibrium constant for this reaction is:\[K_{c} = \frac{[N_{2O}]^2}{[N_2][O_2]}\]
07

Write equation for the formation of ClF3(g)

The formation reaction for chlorotrifluoride, \(ClF_{3(g)}\), is:\[Cl_{2(g)} + 3F_{2(g)} \rightarrow 2ClF_{3(g)}]\]
08

Establish the equilibrium constant expression for ClF3(g)

The equilibrium constant for this reaction is:\[ K_{c} = \frac{[ClF_{3}]^2}{[Cl_{2}][F_{2}]^3}\]

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Most popular questions from this chapter

Write equilibrium constant expressions, \(K_{\mathrm{p}},\) for the reactions (a) \(\mathrm{CS}_{2}(\mathrm{g})+4 \mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{CH}_{4}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{S}(\mathrm{g})\) (b) \(\mathrm{Ag}_{2} \mathrm{O}(\mathrm{s}) \rightleftharpoons 2 \mathrm{Ag}(\mathrm{s})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g})\) (c) \(2 \mathrm{NaHCO}_{3}(\mathrm{s}) \rightleftharpoons\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\)

For which of the following reactions would you expect the extent of the forward reaction to increase with increasing temperatures? Explain. (a) \(\quad \mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{N}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=-90.2 \mathrm{kJ}\) (b) \(\quad \mathrm{SO}_{3}(\mathrm{g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=+98.9 \mathrm{kJ}\) (c) \(\mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=-95.4 \mathrm{kJ}\) (d) \(\mathrm{COCl}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=+108.3 \mathrm{kJ}\)

If the volume of an equilibrium mixture of \(\mathrm{N}_{2}(\mathrm{g}), \mathrm{H}_{2}(\mathrm{g})\) and \(\mathrm{NH}_{3}(\mathrm{g})\) is reduced by doubling the pressure, will \(P_{\mathrm{N}_{2}}\) have increased, decreased, or remained the same when equilibrium is re established? Explain. $$\mathrm{N}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{g})$$

Write an equilibrium constant, \(K_{\mathrm{p}},\) for the formation from its gaseous elements of (a) 1 mol \(\mathrm{NOCl}(\mathrm{g})\) (b) \(2 \mathrm{mol} \mathrm{ClNO}_{2}(\mathrm{g}) ;\) (c) \(1 \mathrm{mol} \mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{g}) ;\) (d) \(1 \mathrm{mol}\) \(\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{s})\)

The Deacon process for producing chlorine gas from hydrogen chloride is used in situations where \(\mathrm{HCl}\) is available as a by-product from other chemical processes. $$\begin{aligned} 4 \mathrm{HCl}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})+2 \mathrm{Cl}_{2}(\mathrm{g}) & \\ \Delta H^{\circ}=&-114 \mathrm{kJ} \end{aligned}$$ A mixture of \(\mathrm{HCl}, \mathrm{O}_{2}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{Cl}_{2}\) is brought to equilibrium at \(400^{\circ} \mathrm{C}\). What is the effect on the equilibrium amount of \(\mathrm{Cl}_{2}(\mathrm{g})\) if (a) additional \(\mathrm{O}_{2}(\mathrm{g})\) is added to the mixture at constant volume? (b) \(\mathrm{HCl}(\mathrm{g})\) is removed from the mixture at constant volume? (c) the mixture is transferred to a vessel of twice the volume? (d) a catalyst is added to the reaction mixture? (e) the temperature is raised to \(500^{\circ} \mathrm{C} ?\)
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