The appropriate answer is option E. Gibbs free energy can be expressed using the equation: ΔG = ΔH - TΔS, where ΔH denotes the change in enthalpy of the reaction, T is the reaction temperature, and ΔS signifies entropy change. For our calculations, we have ΔH = -720.5 kJ/mol which converts to -720500 J/mol (given that 1 kJ = 1000 J), ΔS = -263.7 J/K, and T = 141.0°C, which equals 414.15 K. Consequently, the Gibbs free energy for the specified reaction at 141.0°C is calculated as -611.3 kJ/mol.
Laws of Nature should be differentiated from Scientific and Natural Laws. The Necessitarian Theory suggests that Laws of Nature are those principles which influence the natural phenomena in the universe, meaning the natural world adheres to them.
Given the mass of 
=25.6 g
The molar mass of =390.35g/mol
Conversion of mass of to moles:
Conversion of moles to moles of sulfur:
Conversion of moles of sulfur to individual sulfur atoms using Avogadro's number:
1 mol = 
Density is calculated as mass divided by volume.
Step one:
Convert m³ to ml.
1 m³ = 1,000,000 ml
0.250 m³ x 1,000,000 = 250,000 ml
Step two: Convert mg to g.
1 mg = 0.001 g, hence 4.25 x 10^8 mg equals 0.459 g.
Consequently, the density comes out to be 0.459 g/250,000 = 1.836 x 10^-6 g/ml.
Answer: The change in enthalpy will be -13.
Explanation:-
Endothermic reactions absorb heat, while exothermic reactions release heat. In the case of an endothermic reaction, the change in enthalpy is represented as positive, whereas for an exothermic reaction, it is negative.
When one mole of A combines with one mole of B to form three moles of C
So the stoichiometric ratio being halved also results in the enthalpy for the reaction being halved.
Thus, for this reaction:
The resulting change in enthalpy is -13.
