Question

Вычислить константу равновесия реакции при стандартных условиях KClO4 (кр) ↔ KCl (кр) + 2 O2 (г) , если ∆Н0 р = 33 кДж, ∆S0р = 343 Дж/К и установить в каком направлении она протекает

Answer 1

Ответ:

ΔG=ΔH-TΔS=33*10^3-298*343=-69*10^3 Дж

ΔG<0 - реакция идет при стандартных условиях

ΔG=-RTlnK

K=e^(-ΔG/(RT))=2,71^(69*10^3/(8,314*298))=1,24*10^12

K>>1 - реакция протекает преимущественно в прямом направлении

Answer 2

Calculation of Equilibrium Constant (K) for the Reaction KClO4 (s) ↔ KCl (s) + 2 O2 (g)

To calculate the equilibrium constant (K) for the given reaction, we need to use the equation:

K = e^(-∆G°/RT)

where: - K is the equilibrium constant - ∆G° is the standard Gibbs free energy change - R is the gas constant (8.314 J/(mol·K)) - T is the temperature in Kelvin

Since we are given the standard enthalpy change (∆H°) and the standard entropy change (∆S°), we can use the equation:

∆G° = ∆H° - T∆S°

to calculate the standard Gibbs free energy change (∆G°).

Given: - ∆H° = 33 kJ - ∆S° = 343 J/K

We need to convert the units of ∆H° and ∆S° to J and K, respectively, before using the equation.

Converting units: - ∆H° = 33 kJ = 33,000 J - ∆S° = 343 J/K

Now, we can substitute the values into the equation to calculate ∆G°:

∆G° = ∆H° - T∆S°

At standard conditions, the temperature (T) is 298 K.

∆G° = 33,000 J - (298 K)(343 J/K) ∆G° = 33,000 J - 102,214 J ∆G° = -69,214 J

Now that we have the value of ∆G°, we can calculate the equilibrium constant (K) using the equation:

K = e^(-∆G°/RT)

Substituting the values:

K = e^(-(-69,214 J)/(8.314 J/(mol·K) * 298 K))

Calculating the value of K using a calculator or software, we find:

K ≈ 1.08 x 10^11

Therefore, the equilibrium constant (K) for the reaction KClO4 (s) ↔ KCl (s) + 2 O2 (g) at standard conditions is approximately 1.08 x 10^11.

Direction of the Reaction

To determine the direction in which the reaction proceeds, we can use the value of the equilibrium constant (K).

If K > 1, it indicates that the products are favored at equilibrium, and the reaction proceeds in the forward direction.

If K < 1, it indicates that the reactants are favored at equilibrium, and the reaction proceeds in the reverse direction.

In this case, since the equilibrium constant (K) is very large (K ≈ 1.08 x 10^11), it suggests that the products (KCl and O2) are highly favored at equilibrium. Therefore, the reaction KClO4 (s) ↔ KCl (s) + 2 O2 (g) predominantly proceeds in the forward direction.

Please note that the direction of the reaction can also be influenced by factors such as concentration, pressure, and temperature. The given information assumes standard conditions.