What is the electronic configuration of copper ??
2 answers:
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Answer : The concentration of HI (g) at equilibrium is, 0.643 M
Explanation :
The given chemical reaction is:
Initial conc. 0.10 0.10 0.50
At eqm. (0.10-x) (0.10-x) (0.50+2x)
As we are given:
The expression for equilibrium constant is:
Now put all the given values in this expression, we get:
x = 0.0713 and x = 0.134
We are neglecting value of x = 0.134 because the equilibrium concentration can not be more than initial concentration.
Thus, we are taking value of x = 0.0713
The concentration of HI (g) at equilibrium = (0.50+2x) = [0.50+2(0.0713)] = 0.643 M
Thus, the concentration of HI (g) at equilibrium is, 0.643 M
Answer : The concentration of at equilibrium are 0.132 M, 0.232 M and 0.168 M respectively.
Explanation :
The given chemical reaction is,
First we have to calculate the equilibrium constant for the reaction.
The relation between the equilibrium constant and standard free‑energy is:
where,
= standard free‑energy change = -4.20 kJ/mole
R = universal gas constant = 8.314 J/mole.K
k = equilibrium constant = ?
T = temperature =
Now put all the given values in the above relation, we get:
Now we have to calculate the concentrations of A, B, and C at equilibrium.
The given equilibrium reaction is,
Initially 0.30 0.40 0
At equilibrium (0.30-x) (0.40-x) x
The expression of equilibrium constant will be,
By solving the term x, we get
From the values of 'x' we conclude that, x = 0.716 can not more than initial concentration. So, the value of 'x' which is equal to 0.716 is not consider.
The value of x will be, 0.168 M
The concentration of at equilibrium = (0.30-x) = 0.30 - 0.168 = 0.132 M
The concentration of at equilibrium = (0.40-x) = 0.40 - 0.168 = 0.232 M
The concentration of at equilibrium = x = 0.168 M