Calculate Kp for the following (R = 0.08206 L.atm/mol.K): a) N2O4(g) -2NO2(g) Kc = 5.9 x...

Question

Calculate K_p for the following (R = 0.08206 L.atm/mol.K):

a) N₂O₄(g) ->2NO₂(g) Kc = 5.9 x 10 -3 (at 298 K)

b) N₂(g) + O₂(g) -> 2NO(g) Kc = 4.10 x 10 -31 (at 298 K) [su_box title="♦ Relevant knowledge" box_color="#2d6ff7" radius="1"]

Each gaseous species of an reversible reaction process has the partial pressure parameter. The system's overall pressure is determined by the partial pressures. When the system is in equilibrium then equilibrium is reached. The constant K_p and its equation are used to compare to the same set of partial pressures present. It is important to note that the K_p value can only change in relation to temperature, and it can also change with the volume of the reaction. Thus, at a certain volume and temperature, initially, the partial pressure have to increase until they reach an equilibrium that is compatible with an expression with a quotient of K_p.

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Rhys Roberts · Accepted Answer

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