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### Topic: Chemical Thermodynamics  (Read 855 times)

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#### LocktheRock

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##### Chemical Thermodynamics
« on: April 16, 2021, 01:23:15 PM »

Reaction 1:   A2 (g)  +  B2 (g) ⇄ 2 AB (g)     ΔH0rx = 20 kJ/mole     ΔS0298 = 80 J/mole K

(a) Is this reaction thermodynamically favored (spontaneous) under standard conditions? Justify your answer with a calculation. (Find ΔG0)

(b) Determine the value of the equilibrium constant (Keq) for this reaction at 298 K

(c) If 1 mole of A2, 1 mole of B2, and 1 mole of AB are all placed into a 1 L container at standard conditions, what will happen (increase, decrease, nothing)  to the moles of AB in the container? Justify your answer.

Reaction 2:   X2 (g)  +  Y2 (g)  ⇄  2 XY (g)     ΔH0rx = 60 kJ/mole     ΔS0298 = 100 J/mole K

(d)  Given Y2 (l) ⇄ Y2 (g)  ΔH0rx = 10 kJ/mole

Determine  ΔH0rx  for   X2 (g)  +  Y2 (l)  ⇄  2 XY (g)

Reaction 3:   A2 (g) +  X2 (g)  ⇄  2 AX (g)   @ 298  Keq = 1.5 x 10-7     ΔH0rx = 50 kJ/mole

(e) Is the reaction exothermic or endothermic? Explain.

(f) Calculate the value of ΔS0298  for reaction 3.

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