1)Phosphorus pentachloride decomposes according to the chemical equation,A 0.170 mol sample of PCl5(g) is injected into an empty 2.10 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. Kc=1.80 at 250 C
2)Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2+C-CS2. How many grams of CS2(g) can be prepared by heating 19.4 moles of S2(g) with excess carbon in a 8.40 L reaction vessel held at 900 K until equilibrium is attained? Kc-9.40 at 900K
1)
molarity of PCl5 = 0.170 / 2.10 = 0.081 M
Kc = 1.80
PC5 ------------------> PCl3 + Cl2
0.081 0 0 ----------------> initial
0.081-x x x -----------------> equilibrium
Kc = [PCl3][Cl2]/[PCl5]
1.80 = x^2 / 0.081 -x
x^2 + 1.80 x - 0.1457 = 0
x = 0.0776
equilibrium concentrations:
[PCl5] = 0.081 - x = 0.0034 M
[PCl3] = x =0 .0776 M
[Cl2] = x =0 .0776 M
2 )
molarity of S2 = 19.4 / 8.40 = 2.31 M
S2 (g) + C (s) --------------------> CS2
2.31 -x x
Kc = x / 2.31 -x
9.40 = x / 2.31 -x
21.71 - 9.40 x = x
21.71 = 10.40 x
x = 2.087
molarity of CS2 formed = 2.087 M
moles = molarity x volume
= 2.087 x 8.40
= 17.53
mass = 17.53 x 76
mass = 1332.6 g
mass of CS2 formed = 1332 .6 g
Get Answers For Free
Most questions answered within 1 hours.