Question #128284

Consider the following reversible reaction occurring in a 1.00 L enclosed vessel:

(NH4)2SO4(s) 2NH3(g) + H2SO4(g)

Given that the value of the equilibrium constant, Kc, of this reaction is 2.57 × 10-5, calculate the molar concentrations of NH3(g) and H2SO4(g) at equilibrium. No NH3(g) and H2SO4(g) were present initially.

(NH4)2SO4(s) 2NH3(g) + H2SO4(g)

Given that the value of the equilibrium constant, Kc, of this reaction is 2.57 × 10-5, calculate the molar concentrations of NH3(g) and H2SO4(g) at equilibrium. No NH3(g) and H2SO4(g) were present initially.

Expert's answer

In the equilibrium constant we take into account only gaseous components. Thus, equilibrium constant can be writen as:

"K_{c} = c^{2}(NH_{3})\\times c(H_{2}SO_{4})"

"c(NH_{3}) = 2c(H_{2}SO_{4})"

"(2c)^{2}c=K_{c}=2.57\\times10^{-5}"

"c(H_{2}SO_{4})= (\\frac{2.57\\times10^{-5}}{4})^{\\frac{1}{3}}=0.0186\\frac{mol}{L}"

"c(NH_{3})=0.0186\\times 2 = 0.0372\\frac{mol}{L}"

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