The equilibrium constant for the reaction, H2(g) + I2(g) ⟷2HI(g) is
54.9 at 699.0 K.
What is the equilibrium constant for 4HI(g) ⟷2H2(g) + 2I2(g) under the same conditions?
H2(g) + I2(g) ⟷2HI(g) .......Keq = 54.9 at 699.0 K.
So 2HI ==> H2 + I2 is the reverse and Keq = (1/54.9) and
4HI(g) ⟷2H2(g) + 2I2(g) 4HI(g).....Keq = (1/54.9)^2
Use the excerpt Proposed Equal Rights Amendment (ERA) to answer the question.
The excerpt illustrates the connection of the women's movement to the (Explain)
A. peace movement
B. civil rights movement
C. environmental movement
D. Native American rights movement
B. civil rights movement.
To find the equilibrium constant for the reaction 4HI(g) ⟷ 2H2(g) + 2I2(g), we can use the concept of stoichiometry and the known equilibrium constant for the reaction H2(g) + I2(g) ⟷ 2HI(g).
The equilibrium constant for a reaction is a dimensionless quantity that represents the ratio of the concentrations of products to reactants at equilibrium. It is determined by the stoichiometry of the reaction and the temperature.
In the given reaction, the stoichiometric coefficients are as follows:
H2(g) + I2(g) ⟷ 2HI(g)
To determine the equilibrium constant for the reaction 4HI(g) ⟷ 2H2(g) + 2I2(g), we can use the stoichiometric relationship.
Since 4HI(g) is formed from 2HI(g), we can say that the equilibrium constant for the reaction 4HI(g) ⟷ 2HI(g) is the square of the equilibrium constant for the reaction H2(g) + I2(g) ⟷ 2HI(g).
Therefore, the equilibrium constant for the reaction 4HI(g) ⟷ 2H2(g) + 2I2(g) is (54.9)^2 = 3014.01 at 699.0 K.
To summarize:
Equilibrium constant for H2(g) + I2(g) ⟷ 2HI(g) = 54.9
Equilibrium constant for 4HI(g) ⟷ 2H2(g) + 2I2(g) = (54.9)^2 = 3014.01 at 699.0 K.