Question

a) The equilibrium constant, K_c, for the following reaction is 9.52×10^-2at 350 K.
CH₄(g) + CCl₄(g) -> 2 CH₂Cl₂(g)
Calculate the equilibrium concentrations of reactants and product when 0.251 moles ofCH₄and 0.251 moles of CCl₄are introduced into a 1.00 L vessel at 350 K.

[ CH4]	=	M
[ CCl4]	=	M
[ CH2Cl2]	=	M

b) The equilibrium constant, K_c, for the following reaction is 1.20×10^-2 at 500 K.
PCl₅(g) ->PCl₃(g) + Cl₂(g)  
Calculate the equilibrium concentrations of reactant and products when 0.223 moles of PCl₅(g) are introduced into a 1.00 L vessel at 500 K.  

[PCl5]	=	M
[PCl3]	=	M
[Cl2]	=	M

C) The equilibrium constant, K_c, for the following reaction is 10.5 at 350 K.
2CH₂Cl₂(g) ->CH₄(g) + CCl₄(g)  
Calculate the equilibrium concentrations of reactant and products when 0.313 moles of CH₂Cl₂ are introduced into a 1.00 L vessel at 350 K.

[CH2Cl2]	=	M
[CH4]	=	M
[CCl4]	=	M

Answer 1

iviViali,: o-a51 0.45L - O 3o 854 0 mole ,80 0.033 5 4 6 5 χ = PC5

- 0.0 46076 асн, се as eqili:.313-2x 0.313-2%)2 0.313-2χ 0.135 CH41