The value of the equilibrium constant (Kp) as represented by the first chemical equation is 2.00 x 10-2 at 730 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation.
2HI(g) = H2(g)+I2(g)
H2(g)+I2(g) = 2HI(g)
___ x 10 ____
It's the square root of Kp.
To calculate the value of the equilibrium constant (Kp) for the second equation, we can use the relationship between the equilibrium constants of different reactions.
The second equation is the reverse of the first equation, so the equilibrium constant for the second equation, Kp₂, is related to the equilibrium constant for the first equation, Kp₁, as follows:
Kp₂ = 1 / Kp₁
Given that the value of Kp₁ is 2.00 x 10^(-2), we can substitute this value in the equation to find Kp₂:
Kp₂ = 1 / (2.00 x 10^(-2))
To express the answer in scientific notation, we can simplify the expression:
Kp₂ = 1 / (0.02)
Kp₂ = 50
Therefore, the value of the equilibrium constant (Kp) for the second equation at 730 K is 5.00 x 10^1.