Answer:
The correct answer is option E.
Explanation:
The Gibbs free energy is given by expression:
ΔG = ΔH - TΔS
ΔH = Enthalpy change of the reaction
T = Temperature of the reaction
ΔS = Entropy change
We have :
ΔH = -720.5 kJ/mol = -720500 J/mol (1 kJ = 1000 J)
ΔS = -263.7 J/K
T = 141.0°C = 414.15 K
The Gibb's free energy of the given reaction at 141.0°C is -611.3 kJ/mol.
Answer:
Explanation:
Hello.
In this case, since the molecular formula of the given alcohol is C₄H₁₀O (molar mass = 74.14 g/mol), we can write its combustion reaction as shown below:
Thus, since there is a 1:4 mole ratio with carbon dioxide (molar mass = 44..01 g/mol) and a 1:5 mole ratio with water (molar mass = 18.02 g/mol), we can compute the obtained masses as shown below:
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