2H2S(g)---2H2(g) + S2 delta H=220KJ
k eq is 0.40
a 10.0L vessel containing 2.0 mol of H2S, 2.2 mol of H2, and 2.5 mol of S2
Calculate a trail k eq value to see whether the reaction is at equilibrium.
trail k eq =(h2)^2(S2)/(H2S)^2
= (0.22)^2(0.25)/(0.2)^2
= 0.3025 therefor keq < k eq
In which direction must the system move in order to reach equilibrium? why?
The equation must shift rigth because the numerator is not large enough. Since the numerator contains the product more product must be made in order to bring the ratio up to the value of 0.40
To calculate a trial value for the equilibrium constant (Keq) and determine the direction the system must move to reach equilibrium, you can use the stoichiometry and the given amounts of reactants and products. Here's how you can calculate it:
1. Write down the balanced equation for the reaction: 2H2S(g) → 2H2(g) + S2.
2. Determine the initial moles of each species in the reaction:
- H2S: 2.0 mol
- H2: 2.2 mol
- S2: 2.5 mol
3. Calculate the concentrations (in mol/L) of each species by dividing the moles by the volume of the vessel (10.0 L in this case):
- [H2S] = 2.0 mol / 10.0 L = 0.20 M
- [H2] = 2.2 mol / 10.0 L = 0.22 M
- [S2] = 2.5 mol / 10.0 L = 0.25 M
4. Use the concentrations to calculate the trial Keq value using the expression:
Trail Keq = [H2]^2[S2] / [H2S]^2
Plugging in the values:
Trail Keq = (0.22)^2(0.25) / (0.20)^2
Trail Keq ≈ 0.3025
Comparing the trial Keq value to the given Keq value of 0.40, we find that Trail Keq < Keq. This means that the reaction is not at equilibrium.
To determine the direction in which the system must move to reach equilibrium, we look at the relative magnitudes of the Keq and the trial Keq values. In this case, since Trail Keq < Keq, it suggests that the concentration of the products is lower than it should be at equilibrium.
To reach equilibrium, the system must shift in the direction that produces more products. This means that the reaction must shift to the right, producing more H2 and S2 from H2S, in order to increase the product concentrations and bring the ratio of product to reactant closer to the equilibrium value of Keq.