From the balanced reaction:
1 answer:
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<u>Answer:</u> The value of for the reaction is 6.32 and concentrations of
is 0.094 M, 0.094 M and 0.106 M respectively.
<u>Explanation:</u>
Relation of with
is given by the formula:
where,
= equilibrium constant in terms of partial pressure = 3.45
= equilibrium constant in terms of concentration = ?
R = Gas constant =
T = temperature = 500 K
= change in number of moles of gas particles =
Putting values in above equation, we get:
The equation used to calculate concentration of a solution is:
Initial moles of = 1.00 mol
Volume of the flask = 5.00 L
So,
For the given chemical reaction:
Initial: 0.2 - -
At Eqllm: 0.2 - x x x
The expression of for above reaction follows:
Putting values in above equation, we get:
Negative value of 'x' is neglected because initial concentration cannot be more than the given concentration
Calculating the concentration of reactants and products:
Hence, the value of for the reaction is 6.32 and concentrations of
is 0.094 M, 0.094 M and 0.106 M respectively.