2H2S(g)<---> 2H2(g) + S2(g) The value of Kc for the thermal decomposition of hydrogen sulfide is...

2H2S(g)<---> 2H2(g) + S2(g)

The value of Kc for the thermal decomposition of hydrogen sulfide is 2.2x10^-4 at 1400 K. A sample of gas which [H2S]=4.60 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S] in M? Assume no H2 or S2 was present in the original sample.

Expert Solution

2H2S(g)<---> 2H2(g) + S2(g)

I 4.6 0 0

C -2x 2x x

E 4.6-2x 2x x

Kc = [H2]^2[S2]/[H2S]^2

2.2*10^-4 = (2x)^2*x/(4.6-2x)^2

2.2*10^-4 *(4.6-2x)^2 = 4x^3

x = 0.102

[H2S] = 4.6-2x = 4.6-2*0.102 = 4.396M

[H2} = 2x = 2*0.102 = 0.204M

[S2] = x = 0.102M

queen_honey_blossom answered 4 months ago

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].

2H2S (g) = 2H2 (g) + S2 (g) When heated hydrogen sulfide gas decomposes according to...

2H2S (g) = 2H2 (g) + S2 (g) When heated hydrogen sulfide gas decomposes according to the equation above. A 3.40g smple of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 x10-2 mol of S2 (g) is present at equilibrium. a) Write the expression for the equilibrium constant, Kc for the decomposition reaction represented above. b) Calculate the equilibrium concentration in M of H2 (g) and H2S (g)...

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

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S][H2][S2]===4.50×10−4M0.00M0.00M Find the equilibrium concentration of S2.

Part A The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations:...

Part A The reaction 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7, at 800∘C is carried out with the following initial concentrations: [H2S] = 0.150 M , [H2] =0.200 M , and [S2] = 0.000 M. Find the equilibrium [S2]. Express your answer with the appropriate units.

The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...

The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.150 M , [H2] =0.375 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].

The decomposition of solid ammonium hydrogen sulfide to form ammonia gas and hydrogen sulfide gas is...

The decomposition of solid ammonium hydrogen sulfide to form ammonia gas and hydrogen sulfide gas is an endothermic process.A 6.1589-g sample of the solid is placed in an evacuated 4.000-L vessel at 24.00C.After equilibrium is established, the total pressure inside the vessel is 0.709 bar and some of the solid remains in the vessel. a.Calculate KP for the reaction. b.Calculate the percent of the solid that has decomposed. c.If the system was at equilibrium and the volume of the container...

2 h2s(l) ⇌ 2h2(g) + s2(g) (Kc at 700c is 9.30x10^-8) A) Write the equilibrium expression...

2 h2s(l) ⇌ 2h2(g) + s2(g) (Kc at 700c is 9.30x10^-8) A) Write the equilibrium expression for this reaction B) If 0.45 mol of H2S gas is placed in a 3 L container at 700C what is the concentration, in mol/L, of hydrogen gas when equilibrium is reached.

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌...

Kc for the reaction of hydrogen and iodine to produce hydrogen iodide. H2(g) + I2(g) ⇌ 2HI(g) is 54.3 at 430°C. Calculate the equilibrium concentrations of H2, I2, and HI at 430°C if the initial concentrations are [H2] = [I2] = 0 M, and [HI] = 0.547 M. [H2]= [I2]= [HI]=

Hydrogen sulfide decomposes according to the following reaction,for which Kc = 9.30 multiplied by 10-8 at...

Hydrogen sulfide decomposes according to the following reaction,for which Kc = 9.30 multiplied by 10-8 at 700°C. 2 H2S(g) reverse reaction arrow 2H2(g) + S2(g) If 0.29 mol H2S is placed in a 3.0 L container, what is the equilibrium concentration of H2(g) at 700°C?

For the reaction HI(g) <----> 1/2H2(g) + 1/2I2(g) at 458 C Kc=0145. If a 1.00L vessel...

For the reaction HI(g) <----> 1/2H2(g) + 1/2I2(g) at 458 C Kc=0145. If a 1.00L vessel contains 0.355 mole H2(g), 0.355 mole I2(g), and 1.25 mole HI(g) is this reaction at equilibrium, and if not how will it shift Calculate Kc for H2(g) + I2(g) <----> 2HI(g)

Question