Homework Sourse1Consider the following unbalanced reaction H2 g F2 g HF2 g
1.Consider the following unbalanced reaction: H2 (g) + F2 (g) HF2 (g) : with a Kp = 1.15 * 102 at 25oC
a.If 4.500 mol of H2 are mixed with 6.000 mol of F2 in a 3.000L reaction chamber, determine the equilibrium concentrations of each molecule
b.If this were an exothermic reaction, how would increasing the temperature alter the equilibrium constant?
1.Consider the following unbalanced reaction: H2 (g) + F2 (g) HF2 (g) : with a Kp = 1.15 * 102 at 25oC
a.If 4.500 mol of H2 are mixed with 6.000 mol of F2 in a 3.000L reaction chamber, determine the equilibrium concentrations of each molecule
b.If this were an exothermic reaction, how would increasing the temperature alter the equilibrium constant?
1.Consider the following unbalanced reaction: H2 (g) + F2 (g) HF2 (g) : with a Kp = 1.15 * 102 at 25oC
a.If 4.500 mol of H2 are mixed with 6.000 mol of F2 in a 3.000L reaction chamber, determine the equilibrium concentrations of each molecule
b.If this were an exothermic reaction, how would increasing the temperature alter the equilibrium constant?
Solution
1)
concentration of H2 = 4.500 / 3 = 1.500 M
concentration of F2 = 6.000 / 3.0 = 2.00 M
H2 (g) + F2 (g) <---------------> 2 HF (g)
1.50 2.0 0
1.50 - x 2.0 - x 2x
Kp = (2x)^2 / (1.50 - x) (2 - x)
115 = 4x^2 / x^2 - 3.5x + 3
x = 1.39
Equilibrium concentration :
[H2] = 0.1100 M
[F2] = 0.6100 M
[HF] = 2.780 M
b)
for exothermic reaction , increasing temperature , decreasing the equilibrium constant .
decrease the equilibrium constant
