The following reaction was performed in a sealed vessel at 797 C : H2(g)+I2(g)2H

Question

The following reaction was performed in a sealed vessel at 797 C :

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

Initially, only H2 and I2 were present at concentrations of [H2]=3.15M and [I2]=2.75M. The equilibrium concentration of I2 is 0.0700 M . What is the equilibrium constant, Kc, for the reaction at this temperature?

Express your answer numerically.

The following reaction was carried out in a 3.75 L reaction vessel at 1100 K:

C(s)+H2O(g)CO(g)+H2(g)

If during the course of the reaction, the vessel is found to contain 8.50 mol of C, 12.7 mol of H2O, 4.00 mol of CO, and 6.20 mol of H2, what is the reaction quotient Q?

Enter the reaction quotient numerically.

Consider the reaction

CO(g)+NH3(g)HCONH2(g),    Kc=0.810

If a reaction vessel initially contains only CO and NH3 at concentrations of 1.00 M and 2.00 M, respectively, what will the concentration of HCONH2 be at equilibrium?

Express your answer with the appropriate units.

Consider the following reaction:
HC2H3O2(aq)+H2O(l)H3O+(aq)+C2H3O2(aq)
Kc=1.8×105 at 25C

Part A

If a solution initially contains 0.230 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25C?

Express your answer using two significant figures.

Explanation / Answer

The equilibrium eqn for the reaction is

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

The equilibrium expression for this reaction is Kc= [HI]2 / [H2][I2]

Now let us create the ICE chart

[H2] [I2] [HI]

Initial 3.15M   2.75M 0

Change in conc. x x 2x

Equilibrium conc. 3.15M-x (2.75-x)=0.07 M 0+2x

The value of x= 2.75 - 0.0700 = 2.68 M, therefore completing the ICE chart as

[H2] [I2] [HI]

Initial 3.15M 2.75M 0

Change in conc. 2.68 2.68 5.36

Equilibrium conc. 0.47M 0.07 M 5.36M   

Sustituting the values in eqn, Kc= 5.362 / (0.47)(0.07) = 28.73/0.0329 = 8.73 x102

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