When heated, hydrogen sulfide gas decomposes according to the equation: 2H2S(g)  2 H2(g) + S2(g) A 3.75 gram sample of H2S(g) is introduced into an evacuated rigid 0.75 L container. The sealed container is heated to 483 K and 2.42 x 10 –2 mol of S2 gas is present at equilibrium. a. Write the expression for the equilibrium constant, Kc, for the reaction above.

Explanation:

Moles of   =

Volume of solution = 0.75  L

Initial concentration of =

Equilibrium concentration of =

The given balanced equilibrium reaction is,

Initial conc.              0.15 M        0        0

At eqm. conc.     (0.15-2x) M   (2x) M   (x) M

The expression for equilibrium constant for this reaction will be,

Now put all the given values in this expression, we get :

Given : x = 0.032 M

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the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.