1) The following reaction was performed in a sealed vessel at 786?C : H2(g)+I2(g

Question

1) The following reaction was performed in a sealed vessel at 786?C :

H2(g)+I2(g)?2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.90M and [I2]=3.00M. The equilibrium concentration of I2 is 0.0800M . What is the equilibrium constant, Kc, for the reaction at this temperature?

2)

A mixture initially contains A, B, and C in the following concentrations: [A] = 0.300M , [B] = 0.950M, and [C] = 0.700M . The following reaction occurs and equilibrium is established:

A+2B?C

At equilibrium, [A] = 0.170M and [C] = 0.830M . Calculate the value of the equilibrium constant, Kc.

Express your answer numerically.

3) The following reaction was performed in a sealed vessel at 786?C :

H2(g)+I2(g)?2HI(g)

Initially, only H2 and I2 were present at concentrations of [H2]=3.90M and [I2]=3.00M. The equilibrium concentration of I2 is 0.0800M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Explanation / Answer

Kc=[HI]^2/([H2][I2])
[I2]=0.08
=> [HI]=(3-0.08)*2=5.84
[H2]=3.90-2.92=0.98

Kc=5.84^2/0.08*0.98=435.02

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