If the initial concentration of F(g) is 8.285 mol/L, calculate the % decomposition of F(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kc at 927.0 °C is 370.00. The initial concentration of the reaction products is 0 mol/L.

Question

If the initial concentration of F(g) is 8.285 mol/L, calculate the % decomposition of F(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kc at 927.0 °C is 370.00. The initial concentration of the reaction products is 0 mol/L.

2F(g) = F2(g)

Answer 1

You have the balanced equation.

Set up an ICE chart, substitute into Kc and solve.
initial:
F = 8.285 M
F2 = 0

change:
F2 = +x
F = -2x

equilibrium:
F = 8.285-2x
F2 = x

Answer 2

i don't understand..

Answer 3

To calculate the % decomposition of F(g) when the reaction comes to equilibrium, we need to use the equilibrium constant (Kc) and the initial and final concentrations of F(g).

First, let's identify the balanced equation for the reaction:

2F(g) → F2(g)

According to the balanced equation, for every 2 moles of F(g) that react, we get 1 mole of F2(g) at equilibrium.

Given:
Initial concentration of F(g) = 8.285 mol/L
Initial concentration of F2(g) = 0 mol/L
Kc = 370.00

Let's assume at equilibrium x moles of F(g) decomposed to form x/2 moles of F2(g).

Since the initial concentration of F(g) is 8.285 mol/L and the concentration of F2(g) at equilibrium is 0 mol/L, we know that 8.285 - x is the concentration of F(g) at equilibrium.

Using the formula for Kc:

Kc = [F2(g)] / [F(g)]^2

Substituting the given values at equilibrium:

370.00 = (x/2) / (8.285 - x)^2

Rearranging the equation:

370.00 * (8.285 - x)^2 = x/2

Expanding:

370.00 * (8.285 - x)(8.285 - x) = x/2

Simplifying:

370.00 * (68.598225 - 16.57x + x^2) = x/2

370.00 * (68.598225 - 16.57x + x^2) - x/2 = 0

Now we solve this quadratic equation to find the value of x, which represents the amount of F(g) that decomposes at equilibrium.

Since this equation requires solving a quadratic equation, we will use the quadratic formula:

x = (-b ± sqrt(b^2 - 4ac)) / 2a

In this case, a = 1/2, b = -68.598225, c = 12803.55.

x = (-(-68.598225) ± sqrt((-68.598225)^2 - 4*(1/2)*12803.55)) / (2*(1/2))

Simplifying:

x = (68.598225 ± sqrt(4706.785951 - 25607.1)) / 1

x = (68.598225 ± sqrt(-20800.314049)) / 1

Since the square root of a negative number is not possible in this case, it means that the reaction does not reach equilibrium under the given conditions. Therefore, we cannot calculate the % decomposition of F(g).

However, if you had values that allowed calculation of x, the % decomposition of F(g) would be given by:

% decomposition of F(g) = (x / initial concentration of F(g)) * 100