Question

1)Phosphorus pentachloride decomposes according to the chemical equation,A 0.170 mol sample of PCl5(g) is injected into...

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

Homework Answers

Answer #1

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

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