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) Consider the following reaction:
CO(g)+2H2(g)?CH3OH(g)
A reaction mixture in a 5.15?L flask at a certain temperature contains 26.9g CO and 2.32g H2. At equilibrium, the flask contains 8.67g CH3OH.

Calculate the equilibrium constant (Kc) for the reaction at this temperature.

Explanation / Answer

Ans-1)Kc=(o.o8^2)/(3*3.9)

=0.0000547

Ans-2)Kc=0.7/(0.3*0.95^2)

=2.58

Ans-3) moles CH3OH at equilibrium = 8.65 g ( 1 mol/ 32.042 g)=0.270
[CH3OH] at equilibrium = 0.270 mol/ 5.22 L=0.0517 M

initial moles CO = 26.9 g ( 1 mol/ 28.01 g)=0.960
initial concentration CO = 0.960/ 5.22 =0.184 M

initial moles H2 = 2.32 g ( 1 mol/ 2.016 g)=1.15
initial concentration H2 = 1.15 / 5.22 =0.220 M

CO + 2 H2 < ==> CH3OH
start
0.184 .. 0.220
change
-x . . . -2x . . . . . . +x

x = [CH3OH]= 0.0517
2x = 0.103

[CO]= 0.184 - 0.0517=0.132 M
[H2] = 0.220 - 0.103 = 0.117 M

Kc = 0.0517 / (0.132)( (0.117)^2= 28.6

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