the following reaction may be used to remove sulfur compounds from power plant smokestack emission.
2HS(g) + SO2 >>>> 3S + 2H2O ...... DELTA h = -145 KJ
the value of the euilibrium constant for this reaction is 8.0*10^15 at 25 degree celsius.
a). given the value of K, is this reaction an effective way to clean smokestack emissions of sulfur compounds.?
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To determine whether the reaction is an effective way to clean smokestack emissions of sulfur compounds, we need to compare the value of the equilibrium constant (K) to determine the direction of the reaction at equilibrium.
The equilibrium constant (K) is a measure of the ratio of the concentrations (or pressures) of the products to the concentrations (or pressures) of the reactants, raised to the power of their stoichiometric coefficients.
In this case, the balanced equation for the reaction is:
2HS(g) + SO2(g) >>>> 3S(s) + 2H2O(g)
The equilibrium constant expression for this reaction is:
K = [S]^3[H2O]^2 / [HS]^2[SO2]
Given that the value of the equilibrium constant (K) is 8.0 * 10^15, it indicates that the concentration of the products (S and H2O) is significantly higher than the concentration of the reactants (HS and SO2) at equilibrium. In other words, the reaction is highly favored in the forward direction.
Therefore, based on the high value of the equilibrium constant, it can be concluded that this reaction is indeed an effective way to remove sulfur compounds from power plant smokestack emissions.