Suppose have 1/2 mole of H_2S, 3/4 mole of H_2O, 2 moles of H_2, and 1 mole of S
ID: 509370 • Letter: S
Question
Suppose have 1/2 mole of H_2S, 3/4 mole of H_2O, 2 moles of H_2, and 1 mole of SO_2 which are allowed to react in a vessel maintained at a temperature of 300 K and a pressure of 10^4 Pa. (a) Write down a balanced chemical reaction, with H_2S and H2O on one side of the equation. (b) Write down the condition of equilibrium in terms of the chemical potentials. (c) Show that the number of H_2 molecules is given by N_H_2 = 2 - 3 lambda, where lambda is the proportionality constant defined in class, and write similar equations for the other three components. Foe each component, find the value of lambda where N_i vanishes. (d) Show that lambda_max = 2/3 and lambda_min = -3/8. Which components are depleted in these cases? (e) Assume the nominal solution of the equilibrium condition gives lambda = 1/4. What fraction of each component is in the mixture? (f) Suppose that we increase the pressure, and this changes the nominal value of lambda to 0.8. What fraction of each component is in the mixture now?Explanation / Answer
(a) We have compounds= H2S , H2O, SO2 and H2.
If H2S and H2O are on reactants side, then SO2 and H2 will be left on the product side.
So, chemical reaction = H2S + H2O ===> H2 + SO2.
Balance first the oxygen,
H2S + 2H2O ===> H2 + SO2
Balance the hydrogens,
H2S +2 H2O ===> 3H2 + SO2. ( balanced chemical reaction)
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