For chemical reactions involving ideal gases, the equilibrium constant k can be expressed either in terms of the concentrations of the gases (in m) or as a function of the partial pressures of the gases (in atmospheres). in the latter case, the equilibrium constant is denoted as kp to distinguish it from the concentration-based equilibrium constant kc (sometimes referenced as just k).for the reaction 2ch4(g)⇌c2h2(g)+3h2(g) kc = 0.140 at 1778 ∘c . what is kp for the reaction at this temperature? express your answer numerically.

Explanation:

The relation between Kp and Kc is given below:

Where,  

Kp is the pressure equilibrium constant

Kc is the molar equilibrium constant

R is gas constant

T is the temperature in Kelvins

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

For the first equilibrium reaction:

Given: Kc = 0.140

Temperature = 1778 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (1778 + 273.15) K = 2051.15 K  

R = 0.082057 L atm.mol⁻¹K⁻¹

Δn = (3+1)-(2) = 2  

Thus, Kp is:

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