Question

In: Chemistry

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2 (g) +...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is

S2 (g) + C (s) <----> CS2 (g) Kc=9.40 at 900K

How many grams of CS2(g) can be prepared by heating 12.4 moles of S2(g) with excess carbon in a 7.20 L reaction vessel held at 900 K until equilibrium is attained?

Expert Solution

construct the ICE table

here we donot want to consider the concentration of C because it is solide and it is excess

S2 (g) + C (s) <----> CS2 (g)

I 12.4 0

C -x +x

E 12.4-x +x

now equilibrium expression Kc

Kc = [CS2] / [S2]

9.40 = 12.4-x / x

9.4x = 12.4-x

10.4x = 12.4

x = 12.4 / 10.4

x = 1.1923 moles = [CS2]

grams of CS2 = moles of CS2 x molar mass x CS2

= 1.1923 grams x 76.14 gram/mole

=90.7823 grams

queen_honey_blossom answered 2 years ago

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) +C(s) <===>...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) +C(s) <===> CS2(g). Kc=9.40 at 900k How many grams of CS2(g) can be prepared by heating 12.6 moles of S2(g) with excess carbon in a 6.95 L reaction vessel held at 900 K until equilibrium is attained?

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s)...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g) + C(s) <---> CS2(g) How many grams of CS2(g) can be prepared by heating 21.0 moles of S2(g) with excess carbon in a 9.15 L reaction vessel held at 900 K until equilibrium is attained?

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g) ?c=9.40 at...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g) ?c=9.40 at 900 K How many grams of CS2(g) can be prepared by heating 9.66 mol S2(g) with excess carbon in a 5.85 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g) :

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g)?c=9.40 at 900...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)↽−−⇀CS2(g)?c=9.40 at 900 K How many grams of CS2(g) can be prepared by heating 15.6 mol S2(g) with excess carbon in a 7.05 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g) :

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)−⇀↽−CS2(g)Kc=9.40 at 900...

Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)−⇀↽−CS2(g)Kc=9.40 at 900 KS2(g)+C(s)↽−−⇀CS2(g)Kc=9.40 at 900 K How many grams of CS2(g)CS2(g) can be prepared by heating 16.5 mol S2(g)16.5 mol S2(g) with excess carbon in a 9.40 L9.40 L reaction vessel held at 900 K until equilibrium is attained? mass of CS2(g)CS2(g):

1. The decomposition reaction of carbon disulfide, CS2, to carbon monosulfide, CS, and sulfur is first...

1. The decomposition reaction of carbon disulfide, CS2, to carbon monosulfide, CS, and sulfur is first order with k = 2.8x10-7 s -1 at 1000˚C. CS2....> CS + S a) What is the half life of this reaction at 1000˚C? b) How many days would pass before a 2.00 g sample of CS2 had decomposed to the extent that 0.75 g of CS2 remains? c) Refer to part b). How many grams of CS would be present after this length...

Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Cl2(g) S2Cl2(g) + CCl4(g)...

Carbon disulfide and chlorine react according to the following equation: CS2(g) + 3Cl2(g) S2Cl2(g) + CCl4(g) When 2.94 mol of CS2 and 5.60 mol of Cl2 are placed in a 2.00-L container and allowed to come to equilibrium, the mixture is found to contain 0.580 mol of CCl4. How many moles of Cl2 are present at equilibrium?

Nitrous oxide, N2O(g), reacts with carbon disulfide, CS2(g) according to the equation below. When performed in...

Nitrous oxide, N2O(g), reacts with carbon disulfide, CS2(g) according to the equation below. When performed in a constant volume bomb calorimeter with a heat capacity of 8.775 kJ °C–1 , the temperature of the calorimeter rises from 22.5 °C to 29.1 °C and forms 2.48 g of sulfur, S8. Determine the molar internal energy, ∆U, and the molar enthalpy, ∆H (both in kJ mol-1 ) of the following reaction at 25.0 °C. 3 N2O(g) + CS2(l) ® 3 N2(g) +...

The reaction between sulfur gas (S2) and carbon (C) at high temperatures (900C) results in the...

The reaction between sulfur gas (S2) and carbon (C) at high temperatures (900C) results in the formation of carbon disulfide (CS2). The reaction is: C(s) + S2(g) = CS2(g). What is the concentration (in moles in reaction chamber) of CS2(g) at equilibrium if 3.00 moles of S2(g) and excess carbon are initially added to the 1.00 L reaction chamber? The Keq for this reaction is 3.50.

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 5.00×10−2 mol of H2S and 8.75×10−2 mol of H2 at 800∘C. Find the equilibrium concentration of [S2].