For the following reaction at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.261 mol of F2 is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.
1.5 mol pure HOCl is placed in a 2.7 L flask.
At 2200°C, K = 0.050 for the following reaction.
N2(g) + O2(g) 2 NO(g)
What is the partial pressure of NO in equilibrium with N2 and O2 that were placed in a flask at initial pressures of 0.76 and 0.27 atm, respectively?
You didn't post the reaction for the first one.
To calculate the concentrations of all gases once equilibrium is reestablished after adding 0.261 mol of F2, we need to apply the principles of the equilibrium equation.
The given equilibrium reaction is:
H2(g) + F2(g) ⇌ 2HF(g)
Given:
[H2] = 0.0500 M
[F2] = 0.0100 M
[HF] = 0.400 M
First, we need to determine the changes in the concentrations of each species after adding 0.261 mol of F2.
In the balanced equation, the stoichiometry shows that for every 1 mol of F2 consumed, 2 mol of HF is produced. Therefore, when 0.261 mol of F2 is consumed, twice this amount, or 2 * 0.261 = 0.522 mol of HF is produced.
Since HF is consumed in the forward reaction and produced in the reverse reaction, we subtract the change in HF from the initial concentration:
[HF] (after equilibrium) = [HF] (initial) - change in [HF]
= 0.400 M - 0.522 M
= -0.122 M
The negative value indicates that the concentration of HF has decreased after the reaction.
Next, we determine the change in concentrations of H2 and F2 using stoichiometry. Since the stoichiometric coefficient for H2 is 1, we can say that 0.261 mol of F2 is consumed, resulting in a change of -0.261 M for H2. Similarly, the change in F2 concentration is -0.261 M.
[H2] (after equilibrium) = [H2] (initial) + change in [H2]
= 0.0500 M + (-0.261 M)
= -0.211 M
[F2] (after equilibrium) = [F2] (initial) + change in [F2]
= 0.0100 M + (-0.261 M)
= -0.251 M
The negative values for H2 and F2 indicate that their concentrations have decreased after the reaction.
However, it is important to note that concentrations cannot be negative. The negative values obtained above indicate that the concentrations of H2 and F2 have decreased to zero. Therefore, after reestablishing equilibrium, the concentrations of H2 and F2 will be zero.
The equilibrium concentrations of all gases after adding 0.261 mol of F2 are:
[H2] = 0 M
[F2] = 0 M
[HF] = 0.278 M