# Problem: Calculate Kp for each of the following reactions: N2(g) + O2(g) ⇌ 2NO(g); Kc = 4.10 x 10–31 (at 298 K)

###### FREE Expert Solution

We are being asked to calculate Kp for the reaction:

N2(g) + O2(g) ⇌ 2NO(g)

When dealing with equilibrium:

Kc → equilibrium units are in molarity
Kp → equilibrium units in terms of pressure

Kp and Kc are related to one another by the following equation below:

$\overline{){{\mathbf{K}}}_{{\mathbf{p}}}{\mathbf{=}}{{\mathbf{K}}}_{{\mathbf{c}}}{\left(\mathbf{RT}\right)}^{\mathbf{∆}\mathbf{n}}}$

R = gas constant = 0.08206 (Latm)/(molK)
T = temperature, K
Δn = moles of gas products – moles of gas reactants

Calculate Kp:

Given:                        Kc = 4.10 x 10–31
T = 298 K

Reaction:

N2(g) + O2(g) ⇌ 2NO(g)

reactants = 2 moles gas

90% (72 ratings) ###### Problem Details
Calculate Kp for each of the following reactions: N2(g) + O2(g) ⇌ 2NO(g); Kc = 4.10 x 10–31 (at 298 K)

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