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Question:

The value of Kp/Kc for the following reactions at 300K are, respectively:
N2(g) + O2(g) ⇌ 2NO(g)
N2O4(g) ⇌ 2NO2(g)
N2(g) + 3H2(g) ⇌ 2NH3(g)
[At 300K, RT = 24.62 dm³atm/mol]

1,4.1×10⁻⁶dm⁷sm⁻⁵mol⁻⁵,606.0dm⁶atm²mol⁻⁶

606.0dm⁶atn⁶mol⁻⁶,1.65×10⁷dm³atm⁻²mol⁻¹

1,24.61dm³atm/mol,606.0dm⁶atm²mol⁻⁶

1,24.62dm³atm/mol,1.65×10⁷dm¹⁰atm⁻²mol²

Solution:

N2(g) + O2(g) ⇌ 2NO(g)
Δn = 2 - 2 = 0
Kp/Kc = (RT)^Δn = 1
N2O4(g) ⇌ 2NO2(g)
Δn = 2 - 1 = 1
Kp/Kc = RT = 24.62 dm³atm/mol
N2(g) + 3H2(g)⇌ 2NH3(g)
Δn = 2 - 4 = -2
Kp/Kc = (RT)^Δn = (RT)^-2 = (24.62)^-2 = 1.65 × 10⁻³ dm⁻⁶atm⁻²mol²
Therefore, the values of Kp/Kc for the given reactions are respectively 1, 24.62 dm³atm/mol, and 1.65 × 10⁻³ dm⁻⁶atm⁻²mol².