A chemical system within a sealed 1 L reaction vessel is described by the following reversible reaction equation:

2H2S(g) <---> 2H(g) + S2(g)

(a) the reaction quotient intially
(b) the order of concentration of all three components at equilibrium without using calculations
(c) what the size of the reaction quotient indicates regarding the extent of the forward reaction
(d) the quilibrium concentration of sulphur gas if 0.070 mol of hydrogen sulphide gas is intially placed in the vessel

Any help would be appreciated :)

I think you made a typo. I think you meant

2H2S(g) ==> 2H2(g) + S2(g)

a. Qrxn = (H2)^2(S)/(H2S)^2
ASSUMING H2S was placed in the vessel then Qrxn = 0 since 0/any number = 0
b. I know Keq must be very small. At equilibrium, from lowest to highest concn S2, then H2, then H2S.
c. 0 means the forward reaction is minimal.
d. Can't be solved without knowing Kp or Kc.

Sure! Let's go through each part of the question step by step.

(a) To find the reaction quotient initially, we need to write an expression for it using the concentrations of the reactants and products. The reaction quotient (Q) is calculated in the same way as the equilibrium constant (K), but it is calculated at a particular point in time before the reaction has reached equilibrium.

For the given reaction equation: 2H2S(g) ⇌ 2H(g) + S2(g)

The reaction quotient (Q) is calculated by dividing the product of the concentrations of the species on the right-hand side by the product of the concentrations on the left-hand side, each raised to the power of their respective stoichiometric coefficients.

So, initially, the reaction quotient (Q) can be written as:

Q = [H]^2[S2] / [H2S]^2

(b) The order of concentration of all three components at equilibrium can be determined by examining their stoichiometric coefficients in the balanced reaction equation. In this case, we have:

2H2S(g) ⇌ 2H(g) + S2(g)

From this equation, we can see that the concentration of H2S will be equal to twice the concentration of H and S2 at equilibrium. Therefore, the order of concentration for the components at equilibrium can be described as:

[H2S]:[H]:[S2] = 1:2:1

(c) The size of the reaction quotient (Q) relative to the equilibrium constant (K) indicates the extent of the forward reaction at a particular point in time.

If Q = K, then the system is at equilibrium, and the forward and reverse reactions occur at equal rates.

If Q < K, then the system is not at equilibrium, and the forward reaction has not proceeded to a significant extent. In this case, the reaction will tend to shift in the forward direction to reach equilibrium.

If Q > K, then the system is not at equilibrium, and the forward reaction has proceeded further than at equilibrium. In this case, the reaction will tend to shift in the reverse direction to reach equilibrium.

(d) To find the equilibrium concentration of sulfur gas (S2) if 0.070 mol of hydrogen sulfide gas (H2S) is initially placed in the vessel, we need to consider the stoichiometry and the balanced reaction equation.

Using the balanced reaction equation: 2H2S(g) ⇌ 2H(g) + S2(g)

We can see that for every 2 moles of H2S consumed, 1 mole of S2 is produced. Therefore, the concentration of S2 at equilibrium will be equal to half the initial concentration of H2S that reacted.

So, if the initial concentration of H2S is 0.070 mol, then the equilibrium concentration of S2 will be 0.070 mol / 2 = 0.035 mol.

I hope this explanation helps you understand how to approach and solve the given questions! Let me know if you have any further questions or need more clarification.