One mole of a real gas is subjected to a process from (2 bar, 30 lit, 300 K) to (2 bar, 50 lit, 400 K)Given : CV = 40 J/mol/K, Cp = 50 J/mol/KCalculate ΔU
Question
Solution
To calculate the change in internal energy (ΔU), we need to use the formula:
ΔU = nCvΔT
where: n = number of moles Cv = molar heat capacity at constant volume ΔT = change in temperature
Given: n = 1 mole Cv = 40 J/mol/K Initial temperature (T1) = 300 K Final temperature (T2) = 400 K
First, calculate the change in temperature:
ΔT = T2 - T1 ΔT = 400 K - 300 K ΔT = 100 K
Then, substitute the values into the formula for ΔU:
ΔU = nCvΔT ΔU = 1 mole * 40 J/mol/K * 100 K ΔU = 4000 J
So, the change in internal energy (ΔU) is 4000 J.
Similar Questions
A gas has a volume of 2.0 dm3 at a pressure of 200 kPa and 30 ℃. Calculate the amount (in mol) of gas present.Give your answer to two significant figures.
Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change ( in kJ) for the process is
One mole of an ideal gas is taken through processes AB, BC and CA as shown in the figure.The heat absorbed in process AC is
How many moles of gas (to 1 decimal place, input value only), are contained in a 54.25 L vessel at a pressure of 173.6 kPa and temperature of 0.2 °C?
What is the average kinetic energy per particle in 1.00 mole of an ideal gas at a pressure of 1.50 atmospheres and a volume of 2.00 liters?
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.