Question

Consider the following chemical equilibrium: +2H2gO2g ⇌ 2H2Ol Now write an equation below that shows how to calculate Kp from Kc for this reaction at an absolute temperature T. You can assume T is comfortably above room temperature. If you include any common physical constants in your equation be sure you use their standard symbols, found in the ALEKS Calculator.K_p=?

Answer 1

Answer:

$K_p= K_c\times (RT)^{-3}$

Explanation:

The relation between Kp and Kc is given below:

$K_p= K_c\times (RT)^{\Delta n}$

Where,  

Kp is the pressure equilibrium constant

Kc is the molar equilibrium constant

R is gas constant , R = 0.082057 L atm.mol⁻¹K⁻¹

T is the temperature in Kelvins

Δn = (No. of moles of gaseous products)-(No. of moles of gaseous reactants)

For the first equilibrium reaction:

$2H_2_{(g)}+O_2_{(g)}\rightleftharpoons2H_2O_{(l)}$

Δn = (0)-(2+1) = -3

Thus, Kp is:

$K_p= K_c\times (RT)^{-3}$