A) The synthesis of methanol from carbon monoxide and hydrogen gas is described

Question

A) The synthesis of methanol from carbon monoxide and hydrogen gas is described by the following chemical equation:

CO(g)+2H2(g)CH3OH(g)

The equilibrium constant for this reaction at 25 Cis Kc=2.3×104. In this trial, you will use the equilibrium-constant expression to find the concentration of methanol at equilibrium, given the concentration of the reactants.

Suppose that the molar concentrations for CO and H2 at equilibrium are [CO] = 0.04 M and [H2] = 0.04 M.

Use the formula you found in Part B to calculate the concentration of CH3OH.

B) Consider the reaction:
CO(g)+H2O(g)CO2(g)+H2(g)
An equilibrium mixture of this reaction at a certain temperature was found to have [CO]= 0.0213 M , [H2O]= 0.0115 M , [CO2]= 0.190 M , and [H2]= 0.0324 M .

What is the value of the equilibrium constant at this temperature?

C)An equilibrium mixture of the following reaction was found to have [I2]= 0.0225 M at 1200 C.

What is the concentration of  I ?
I2(g)2I(g)
Keq= 1.2×102 at 1200 C

Explanation / Answer

1.For the reaction CO(g)+ 2H2(g)<---->CH3OH(g)

K= Equilibrium constant = [CH3OH]/[CO] [H2]2 =2.3*104 ,

Given [CO]=0.04M and [H2]=0.04M

[CH3OH] = 2.3*104*0.04*0.04*0.04=1.472M

2. For the reaction CO(g)+ H2O(g)<--->àCO2(g)+ H2(g)

K= Equilibrium constant = [CO2][H2]/[CO] [H2O]

Given [CO]=0.0213M and [H2O]=0.0115M, [CO2] =0.19 and [H2] = 0.0324

K= 0.19*0.0324/(0.0213*0.0115) =25.13

3. for the reaction I2(g)<--->2I(g)

K= [I]2/[I2] = 1.2*10-2

[I2] =0.0225

[I]2= 1.2*10-2*0.0225, [I] =0.016432M

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