The equilibrium constant, Kc, for the following reaction is 7.00×10-5 at 673 K.
NH4I(s) NH3(g) + HI(g)
Calculate the equilibrium concentration of HI when 0.210 moles of NH4I(s) are introduced into a 1.00 L vessel at 673 K.
[HI] = M
NH4I(s)→ NH3(g)+HI(g)_4I_{(s)}\to\>NH_{3(g)}+HI_{(g)}4I(s)→NH3(g)+HI(g)
kc=[NH3][HI][NH4I]k_c=\frac{[NH_3][HI]}{[NH_4I]}kc=[NH4I][NH3][HI]
7×10−5=(x)(x)0.210−x7×10^{-5}=\frac{(x)(x)}{0.210-x}7×10−5=0.210−x(x)(x)
⟹ x2=1.470×10−5\implies\>x^2=1.470×10^{-5}⟹x2=1.470×10−5
x=3.834×10−3x=3.834×10^{-3}x=3.834×10−3
[HI]=3.834×10−3M[HI]=3.834×10^{-3}M[HI]=3.834×10−3M
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