The value of Keq for the equilibrium
H2 (g) + I2 (g) ↔ 2 HI (g)
is 794 at 25 °C. What is the value of Keq for the equilibrium below?
1/2 H2 (g) + 1/2 I2 (g) ↔ HI (g)
K'eq = sqrt Keq.
To find the value of Keq for the equilibrium equation:
1/2 H2(g) + 1/2 I2(g) ↔ HI(g),
we can use the relationship between Keq values and the chemical equation.
In this case, the given equation is half of the original equation:
H2(g) + I2(g) ↔ 2 HI(g).
To find the Keq value for the given equation, we can square the Keq value of the original equation since the stoichiometric coefficients have been halved:
(Keq of 1/2 H2(g) + 1/2 I2(g) ↔ HI(g))² = Keq of H2(g) + I2(g) ↔ 2 HI(g).
Therefore, the value of Keq for the equilibrium
1/2 H2(g) + 1/2 I2(g) ↔ HI(g)
would be the square root of the given Keq value:
√794 = 28.2 (approximately).
Hence, the value of Keq for the given equilibrium is approximately 28.2.
To find the value of Keq for the given equilibrium, we can use the relationship between the two equilibria.
The balanced chemical equation for the first equilibrium is:
H2 (g) + I2 (g) ↔ 2 HI (g)
Now, let's compare this to the second equilibrium:
1/2 H2 (g) + 1/2 I2 (g) ↔ HI (g)
We can see that the second equilibrium can be obtained by dividing the coefficients of the first equilibrium by 2.
Since Keq is a dimensionless quantity, it remains the same when we adjust the coefficients. Therefore, the value of Keq for the second equilibrium is also 794.
In summary, the value of Keq for the equilibrium: 1/2 H2 (g) + 1/2 I2 (g) ↔ HI (g) is 794.