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, K_c for the decomposition reaction represented above.

b) Calculate the equilibrium concentration in M of H₂ (g) and H₂S (g) in the container 483 K

c) Calculate the value of the equilibrium constant K_c for the decomposition reaction of 483K

Solutions

Expert Solution

K =[ H₂ ]^2 [S₂ ] / [H₂S ] ^2

2H₂S (g) = 2H₂ (g) + S₂ (g)

a) Write the expression for the equilibrium constant, K_c for the decomposition reaction represented above

K =[ H₂]^2 [S₂] / [H₂S ] ^2

b) Calculate the equilibrium concentration in M of H₂ (g) and H₂S (g) in the container 483 K

	H₂S	2H₂	S₂
I		0	0
C	-5.95 X10^-2	5.95 X10^-2	2.98X10^-2
E	2.03 X10^-2	5.95 X10^-2	2.98X10^-2

M of H₂ (g)-------------- 5.95 X10^-2

and H₂S (g)------------------ 2.03 X10^-2

in the

c) Calculate the value of the equilibrium constant K_c for the decomposition reaction of 483K

K =[ 5.95 X10^-2]^2 [2.98X10^-2] / [2.03 X10^-2 ] ^2 = 0.256

queen_honey_blossom answered 1 year ago

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