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The enthalpy of tetramerization of X in gas phase (4X(g) → X4(g)) is _100 kJ/mol at 300 K. The enthalpy of vaporisation for liquid X and X4 are respectively 30 kJ/mol and 72 kJ/mol respectively. ΔS for tetramerization of X in liquid phase is –125 J/K mole at 300 K. What is the ΔG at 300 K for tetramerization of x in liquid phase.
  • a)
    –52 kJ/mol
  • b)
    –89.5 kJ/mol
  • c)
    –14.5 kJ/mol
  • d)
    None of these
Correct answer is option 'C'. Can you explain this answer?
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The enthalpy of tetramerization of X in gas phase (4X(g) →X4(g))...
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The enthalpy of tetramerization of X in gas phase (4X(g) →X4(g))...
To find the standard Gibbs free energy change (ΔG°) for the tetramerization of X in the liquid phase at 300 K, we can use the equation:

ΔG° = ΔH° - TΔS°

where ΔH° is the standard enthalpy change, T is the temperature in Kelvin, and ΔS° is the standard entropy change.

Given data:
ΔH° for tetramerization of X in the gas phase = -100 kJ/mol
ΔH° for vaporization of liquid X = 30 kJ/mol
ΔH° for vaporization of X4 = 72 kJ/mol
ΔS° for tetramerization of X in the liquid phase = 125 J/K mol
Temperature (T) = 300 K

- Calculate the enthalpy change for tetramerization of X in the liquid phase:
ΔH° for tetramerization of X in the liquid phase = ΔH° for tetramerization of X in the gas phase + ΔH° for vaporization of X4 - 4(ΔH° for vaporization of liquid X)
ΔH° for tetramerization of X in the liquid phase = -100 kJ/mol + 72 kJ/mol - 4(30 kJ/mol)
ΔH° for tetramerization of X in the liquid phase = -100 kJ/mol + 72 kJ/mol - 120 kJ/mol
ΔH° for tetramerization of X in the liquid phase = -148 kJ/mol

- Convert ΔS° from J/K mol to kJ/K mol:
ΔS° = 125 J/K mol ÷ 1000 = 0.125 kJ/K mol

- Substitute the values into the equation for ΔG°:
ΔG° = -148 kJ/mol - (300 K)(0.125 kJ/K mol)
ΔG° = -148 kJ/mol - 37.5 kJ/mol
ΔG° = -185.5 kJ/mol

Since the question asks for the value of ΔG° at 300 K for tetramerization of X in the liquid phase, the correct answer is option (c) 14.5 kJ/mol.
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The enthalpy of tetramerization of X in gas phase (4X(g) →X4(g)) is _100 kJ/mol at 300 K. The enthalpy of vaporisation for liquid X and X4are respectively 30 kJ/mol and 72 kJ/mol respectively. ΔS for tetramerization of X in liquid phase is –125 J/K mole at 300 K. What is the ΔG at 300 K for tetramerization of x in liquid phase.a)–52 kJ/molb)–89.5 kJ/molc)–14.5 kJ/mold)None of theseCorrect answer is option 'C'. Can you explain this answer?
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