Question

-The equilibrium constant, K_c, for the following reaction is 5.10×10^-6 at 548 K.

NH₄Cl(s) NH₃(g) + HCl(g)

Calculate the equilibrium concentration of HCl when 0.452 moles of NH₄Cl(s) are introduced into a 1.00 L vessel at 548 K.

[HCl] = _________M

-The equilibrium constant, K_c, for the following reaction is 55.6 at 698 K.

H₂(g) + I₂(g)  2 HI (g)

Calculate the equilibrium concentrations of reactants and product when 0.380 moles of H₂and 0.380 moles of I₂are introduced into a 1.00 L vessel at 698 K.

[ H2]	=	_______M
[ I2]	=	_______M
[ HI ]	=	_______M

THANK YOU

Answer 1

@ Initial concentrations of H, and I, ase; [H₂] = 0.380 mol -0.380M [I] = 0.380 mol = 0.380 M IL IL H₂ cg) + Izeg) - 2H I cq) Initial 0.380 0.380 +22 Change -X Equilibrium 0.380-X 0.380-x 2x Kc = [HI] 2 [H₂] [I ₂ 2 55.6 (0.380-x) (0.380-x) 2 55.6 2 n 0.380-x 7.457 = 2x 0.380-X 2.834-7.457x = 2x 2.834 = 9.457x x - 0.2996M (2x)2 11

of Equilibrium concentrations reactants and products are; [H₂] = 0.380-0.2996 = 0.0804M (1,] - 0.380 -0.2996 = 0.0804M [HI] = 2x 0.2996 = 0.5992M