contestada

When 229 J of energy is supplied as heat to 3.0 mol of nitrogen N2(g) at constant pressure, the temperature of the sample increases by 2.55 K. Assuming that under these conditions nitrogen behaves as an ideal gas, what is the value of the molar heat capacity at constant volume of N2(g)?

Respuesta :

Answer: Molar heat capacity at constant volume of [tex]N_2[/tex] is 64.9 J/Kmol

Explanation:

[tex]C_p-C_v =nR[/tex]

where

[tex]C_p[/tex] = heat capacity at constant pressure

[tex]C_v[/tex] = heat capacity at constant volume

n = number of moles = 3.0

R= gas constant = 8.314 J/Kmol

[tex]Cp =\frac{q}{ΔT}[/tex]

q = heat absorbed

[tex\\Delta T[/tex] = change in temperature = 2.55 K

[tex]Cp =\frac{229J}{2.55K}=89.8J/K[/tex]

Putting in the values:

[tex]89.8_C_v=3.0\times 8.314[/tex]

[tex]C_v=89.8-24.9=64.9J/Kmol[/tex]

Thus molar heat capacity at constant volume of [tex]N_2[/tex] is 64.9 J/Kmol

Otras preguntas