A sample of oxygen is subjected to an absolute pressure of 2.4 atm. If the specific internal energy of the sample at 310 K is 5700 J/mol relative to a known reference state, what is the specific enthalpy of the oxygen relative to that same reference state?

The required specific enthalpy for oxygen = 8277.34 J/mol

Explanation:

Given that :

Pressure = 2.4 atm

Temperature = 310 K

specific internal energy U = 5700 J/mol

To find the specific enthalpy using the formula:

H = U + PV

where;

H is known as the specific enthalpy

Recall that from ideal gas equation

PV = nRT

For specific enthalpy, it is constant that n = 1

Thus;

PV = RT

replacing that into the equation (H = U + PV), we have:

here;

R = 8.314 J/mol K (constant)

H = U + RT

H = 5700 J/mol +( 8.314 J/mol K × 310 K)

H = 5700 J/mol + ( 2577.34 J/mol)

H = 8277.34 J/mol

c. 4.54 x 10–12 j happens to be correct