Calculate the energy required to change the temperature of 1.00 kg of ethane (C2H6) from 25.0"C to 73.4"C in a rigid vessel. (Cv for C2H6 is 44.60 J K%1 mol%1.) Calculate the energy required for this same temperature

Question:

Calculate the energy required to change the temperature of 1.00 kg of ethane (C2H6) from 25.0"C to 73.4"C in a rigid vessel. (Cv for C2H6 is 44.60 J K%1 mol%1.)

Calculate the energy required for this same temperature change at constant pressure.

Calculate the change in internal energy of the gas in each of these processes.

Answer:

The answers are

qv = 71787.16 J

qp = 85169.99 J

ΔE = 71787 J for both constant volume and constant pressure processes

Explanation:

Mass of ethane gas, m = 1.00 kg = 1000 g

Cv = 44.60 J / (K·mol)

The temperature change is given by

ΔT T₂ - T₁ = 73.4 °C - 25 °C = 48.4 °C

The molar mass of ethane = 30.07 g/mol

Number of moles, n of ethane = mass / (molar mass) = 1000/30.07

= 33.26 moles

Therefore the energy required at constant volume to change the temperature of 1.00 kg of ethane (C₂H₆) from 25.0 °C to 73.4 °C

is given by H qv = n ·Cv·ΔT = 33.26 * 44.60*48.4 = 71787.16 J

b) At constant pressure we have Cp - Cv = R

∴ Cp = R + Cv

= 8.3145 + 44.6 = 52.9145 J / (K·mol)

Therefore we have H, qp = n ·Cp·ΔT = 33.26*52.9145*48.4

= 85169.99 J

For constant volume process, we have

q = U

Therefore ΔU = Δq = 71787 J

For constant pressure process, we have

ΔU = n*Cv*dT = 71787 J