Question

The enthalpy of a reaction does not depend upon:
A. The intermediate reaction steps
B. The temperature of initial and final states of the reaction
C. The physical states of reactants and products
D. Use of different reactants for the formation of the same

Answer 1

Hint: The enthalpy change does not depend upon the nature of different steps to bring out a chemical reaction.

Complete step by step answer:
We know that enthalpy is a property of a thermodynamic system, a convenient state function preferred in many measurements in chemical, biological, and physical systems under a constant pressure.
-It is defined as the sum of the internal energy of the system and the product of its pressure and volume. -The term pressure-volume expresses the work required to establish the physical dimensions of a system, that is, by displacing its atmosphere and making room for it.
-As a state function, enthalpy depends only on the final configuration of internal energy, pressure, and volume, and not on the path taken to achieve it.
-The unit of measurement for enthalpy in the International System of Units (SI) is $joule$. Other historical traditional units still in use include the British Thermal Unit $(BTU)$ and calories.
-The temperature of an ideal gas is independent of its pressure, and depends only on its temperature, which is related to its internal energy. Real gases at common temperatures and pressures often understand this behavior closely, which simplifies practical thermodynamic design and analysis.
Hence, the correct option is A.

Note: The enthalpy of a thermodynamic system is defined as the sum of its internal energy $U$ and the work required to obtain its pressure and volume:
$H = U + PV$
Where $P$ is the pressure , and $V$ is the volume of the system.
It does not depend upon the nature of different steps of chemical reaction.