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At 789 K, the equilibria for the following reactions are
CuS(s) + H2(g) → Cu(s) + H2S(g) Kc = 78.9
CS2(g) + H2(g) → CS(g) + H2S(g) Kc = 0.289
Based on the given equilibria, what will be the Kc for CuS (s) + CS (g) → Cu (s) + CS2 (g)?
The dissociation of hydrogen selenide (H2Se) takes place in two steps:
H2Se ⇌ H+ + HSe- K1 = 1.29×10-4
HSe- ⇌ H+ + Se2- K2 = 1.00×10-11
Calculate the equilibrium constant for the following reaction:
Se2- + 2H+ ⇌ H2Se
The following reaction is a vital step in the metabolism of glucose: glucose + ATP ⇌ glucose-6-phosphate + ADP
Determine the equilibrium constant for the above reaction using the related equilibrium constants:
glucose + Pi ⇌ glucose-6-phosphate, K = 3.114 × 10–3
ATP ⇌ ADP + Pi, K = 2.716 × 105
The dissociation of hydrogen selenide (H2Se) takes place in two steps:
H2Se ⇌ H+ + HSe- K1 = 1.29×10-4
HSe- ⇌ H+ + Se2- K2 = 1.00×10-11
Calculate the equilibrium constant for the following reaction:
Se2- + 2H+ ⇌ H2Se
The following equation shows the reaction of hydrogen sulfate anion (HSO4-) with ammonia (NH3) to form sulfate (SO42-) and ammonium ions (NH4+):
HSO4-(aq) + NH3(aq) ⇌ SO42-(aq) + NH4+(aq)
If the value of Ka for HSO4- is 1.26 × 10-2, and the Kb value for NH3 is 1.8 × 10-5, determine whether the value of Kc will be greater than or lower than 1 for this reaction. Also, identify the direction which will be favored at equilibrium.