2H2(g)+S2----------->2H2S
A.)how would the equilibrium be affected given the following:
- increase in temperature=
- increase in hydrogen concetration=
- increase in reaction container volume=
B.) what is equilibrium expression??
please help anywork would be appreciated!!
You need to give the states of S and H2S. You need to show if it is an endo or exothermic reaction. I suggest you make a new post out of it so it will go to the top.
A.) The equilibrium of a reaction can be affected by changes in temperature, concentration, and volume. Let's analyze each scenario:
1. Increase in Temperature: For the given reaction, the formation of hydrogen sulfide (H2S) is exothermic, meaning it releases heat. According to Le Chatelier's principle, when you increase the temperature, the equilibrium will shift in the endothermic direction to absorb the extra heat. In this case, the equilibrium will shift towards the reactants (H2 and S2) to counteract the temperature increase.
2. Increase in Hydrogen Concentration: If you increase the concentration of hydrogen (H2) in the reaction, Le Chatelier's principle states that the equilibrium will shift to reduce the excess of H2. The reaction would move towards the products (H2S) as both reactants (H2 and S2) are consumed to produce more H2S.
3. Increase in Reaction Container Volume: When the volume of the reaction container is increased, the pressure will decrease. If the reaction involves gases, Le Chatelier's principle states that the equilibrium will shift towards the side with more moles of gas to counteract the pressure decrease. In this case, since the reactants have 2 moles of gas (H2 and S2), while the product has only 1 mole of gas (H2S), the equilibrium will shift towards the reactant side to increase the overall pressure.
B.) The equilibrium expression for the given reaction 2H2(g) + S2(g) ⇌ 2H2S(g) is written as follows:
\[ \text{K}_{\text{eq}} = \frac{{[\text{H2S}]^2}}{{[\text{H2}]^2[\text{S2}]}} \]
Where [H2S], [H2], and [S2] represent the molar concentrations of H2S, H2, and S2 gases, respectively, at equilibrium. K_eq is the equilibrium constant, which represents the ratio of the concentrations of the products to the concentrations of the reactants, all raised to their stoichiometric coefficients.