Calculate the equilibrium constant Kp for this reaction, given the following information (at 296 K ): 2NO(g)+Br2(g)⇌2NOBr(g)Kc=1.8 2NO(g)⇌N2(g)+O2(g)Kc=2.3×1030

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 = 1.8

Temperature = 296 K

R = 0.082057 L atm.mol⁻¹K⁻¹

Δn = (2)-(2+1) = -1  

Thus, Kp is:

For the second equilibrium reaction:

Given: Kc =

Temperature = 296 K

R = 0.082057 L atm.mol⁻¹K⁻¹

Δn = (2)-(2) = 0

Thus, Kp is:

i believe the answer is a.

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explanation: