Which of the following statements is true regarding constant pressure heat capacity?

Constant pressure heat capacity, often denoted as ( C_p ), is indeed typically larger than constant volume heat capacity, known as ( C_v ). This is because when heat is added to a substance at constant pressure, not only is energy used to increase the temperature of the substance, but additional energy is also required to do work on the surroundings as the substance expands.

In contrast, at constant volume, all the heat added to the system contributes solely to increasing the internal energy (and hence the temperature) of the system since there is no change in volume and therefore no work is done on the surroundings. This results in ( C_p ) being greater than ( C_v ).

It's crucial to understand that the relationship between these two capacities is expressed in thermodynamics as follows:

[

C_p = C_v + R

]

where ( R ) represents the gas constant for an ideal gas. This relationship indicates that ( C_p ) will always be greater than ( C_v ) for a given gas, making the statement about ( C_p ) being larger than ( C_v ) accurate.

Other statements, such as ( C_p ) being equal to ( C_v ) or not changing with temperature