When CH4(g) (0.06318 mol/L) and 16.43 mol of H2S(g) in a 130.0 L reaction vessel at 711.0 °C are allowed to come to equilibrium the mixture contains 0.04107 mol/L of CS2(g). What is the equilibrium concentration (mol/L) of H2S(g)?
CH4(g)+2H2S(g) = CS2(g)+4H2(g)
This one may be a little different.
i have no clue on how to set this up....
Note here that CH4 is given as mols/L (instead of mols for the other problems)
so if (CH4) = 0.06318 mols/L and the volume is 130.0L, then mols = 0.06318 x 130L = 8.213 mols.
......CH4 + 2H2S ==> CS2 + 4H2
I.....8.213..16.43....0.....0
C.....-x.....-2x......x.....4x
E....8.213-x..16.43-2x..x...4x
And the problem tells you (CS2) = 0.04107 mols/L so that x 130.0 = mols and you go from there.
.04107 x 130 = 5.3391
4x= 5.3391
x = 1.3348
therefore H2S(g) = 1.3348/130
= .01027?
.04107 x 130 = 5.3391 OK here
4x= 5.3391 Why multiply by 4. It's H2S you want, not H2. So H2S mols = 16.43-2x = 16.43 -(2*5.339) = ? and then (H2S) = mols/L.
x = 1.3348
therefore H2S(g) = 1.3348/130
= .01027?
To find the equilibrium concentration of H2S(g), we need to apply the principles of chemical equilibrium and use the given information about the initial and equilibrium concentrations of the other gases.
The balanced equation for the reaction is:
CH4(g) + 2H2S(g) = CS2(g) + 4H2(g)
Let's assign variables for the initial and equilibrium concentrations of CH4(g), H2S(g), and CS2(g):
- Initial concentration of CH4(g): [CH4]₀ = 0.06318 mol/L
- Equilibrium concentration of CH4(g): [CH4] eq
- Initial concentration of H2S(g): [H2S]₀ = 16.43 mol/L
- Equilibrium concentration of H2S(g): [H2S] eq
- Equilibrium concentration of CS2(g): [CS2] eq = 0.04107 mol/L
According to the balanced equation, the ratio in which CH4 reacts with H2S is 1:2. This means that for every 1 mole of CH4 that reacts, 2 moles of H2S will be consumed.
Therefore, we can say:
[H2S] eq = 2 x (Initial moles of CH4 consumed)
To find the initial moles of CH4 consumed, we can use the initial and equilibrium concentrations of CH4 and CS2.
The moles of CH4 consumed can be calculated using the formula:
Initial moles of CH4 consumed = [CH4]₀ - [CH4] eq
We know that the change in the concentration of CH4 (Δ[CH4]) is equal to the initial moles of CH4 consumed, as one mole of CH4 reacts to produce one mole of CS2.
Therefore, Δ[CH4] = [CH4]₀ - [CH4] eq = moles of CH4 consumed = moles of CS2 formed
As per stoichiometry, 1 mole of CS2 is formed for every mole of CH4 consumed. So, we can say:
Δ[CH4] = [CS2] eq = 0.04107 mol/L
Now, we can substitute the values into the equation to find the equilibrium concentration of H2S:
[H2S] eq = 2 x Δ[CH4] = 2 x [CS2] eq = 2 x 0.04107 mol/L
Therefore, the equilibrium concentration of H2S(g) is approximately 0.08214 mol/L.