At 63.5 °C, ethanol (CH₃CH₂OH) has a vapor pressure of 0.526 atm. Determine the K_p and K_c values for the equilibrium CH₃CH₂OH(l) ⇌ CH₃CH₂OH(g) at 63.5 °C.

Consider the following equilibrium:

2NO(g) + Br₂(g) ⇌ 2NOBr(g)

At 600 K, the partial pressures of the three gases in the equilibrium mixture, NO, Br₂, and NOBr, are 0.150 atm, 0.115 atm, and 0.348 atm, respectively.

Determine the value of K_c at this temperature.

The value of K_c for the following reaction 2 NO₂(g) ⇌ N₂O₄(g) is 4.72 at 100°C. Determine its K_p value at this temperature.

What is the change in the number of gas moles (Δn) for each of the following reactions?

I) H_2(g) + Br_2(l) → 2HBr_(g)

II) (NH₄)₂CO_3(s) → 2NH_3(g) + CO_2(g) + H₂O_(g)

III) 3H_2(g) + N_2(g) → 2NH_3(g)

IV) Mg_(s) + I_2(s) → MgI_2(s)

The reaction PH₃BCl₃(s) ⇌ PH₃(g) + BCl₃(g) has K_c = 6.96 × 10^–5 at 60 ºC. Determine the value of K_p.

The reaction 2 NO(g) + Br₂(g) ⇌ 2 NOBr(g) has K_p = 2.40 at 100 ºC. Determine the value of K_c.