If 7.84 × 107 J of energy is released from a fusion reaction, what amount of mass in kilograms would be lost? Recall that c = 3
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Answer : The equilibrium concentrations of all species are, 0.05 M, 0.043 M and 0.975 M respectively.
Explanation : Given,
Moles of = 2 mole
Moles of = 1 mole
Volume of solution = 1 L
Initial concentration of = 2 M
Initial concentration of = 1 M
The given balanced equilibrium reaction is,
Initial conc. 2 M 1 M 0
At eqm. conc. (2-2x) M (1-x) M (2x) M
The expression for equilibrium constant for this reaction will be,
The for reverse reaction =
Now put all the given values in this expression, we get :
By solving the term 'x', we get :
x = 0.975
Thus, the concentrations of at equilibrium are :
Concentration of = (2-2x) M = (2 - 2 × 0.975) M = 0.05 M
Concentration of = (1-x) M = 1 - 0.975 = 0.043 M
Concentration of = x M = 0.975 M
Therefore, the equilibrium concentrations of all species are, 0.05 M, 0.043 M and 0.975 M respectively.