Consider the gas phase reaction 2A(g) + 3B(g) ⇌ 2C(g) at a given temperature. When 2.0 moles of A(g) are reacted with 2.0 moles of B(g), 0.8 moles of C(g) are formed at equilibrium at a total pressure of 2.0 bar. The value of the equilibrium constant, K_P of this reaction at the given temperature is closest to

Concept:

• Thermodynamic equilibrium is an axiomatic concept of thermodynamics. It is an internal state of a single thermodynamic system or a relation between several thermodynamic systems.
• Systems in mutual thermodynamic equilibrium are simultaneously in mutual thermal, mechanical, chemical, and radiative equilibrium

K_p is the equilibrium constant it's calculated from the ratio of partial pressure of products to reactants.

Explanation:-

In the reaction, 2A(g) + 3B(g) ⇌ 2C(g)

the equilibrium constant K_p will be,

• Total number of moles

= 1.2+0.8+0.8

=2.8 mol

P_A= X_A.P_T,
P_B=X_B.P_T,
P_C=X_C.PT, 
P_D=X_D.PT

where, P_A, PB, P_C, and P_D are the partial pressure of gas A, B, C, and D respectively.

X_A, XB, XC, and XD are the mole fraction of gas A, B, C, and D respectively.

P_T is the total pressure of the system.

= 2.4

Conclusion:-

The value of the equilibrium constant, KP of this reaction at the given temperature is closest to 2.4. Hence, option 3 is correct.