Answer:
Q= 6213.72 J
Explanation:
Given that
n = 2.2 moles
T= 490 K
Given that gas is ideal gas and process is isothermal.
We know that internal energy for ideal gas only depends on the temperature.The temperature change in the isothermal process is zero.That is why internal energy change will be zero.
ΔU = 0
From first law of thermodynamics
Q = ΔU + W
Q= W
We know that work for isothermal process
[tex] W=P_1V_1\ln \dfrac{P_1}{P_2}[/tex]
[tex] W=nRT\ln \dfrac{V_2}{V_1}[/tex]
Given that V₂ = 2 V₁
[tex] W=nRT\ln \dfrac{2V_1}{V_1}[/tex]
[tex] W=nRT\ln 2[/tex]
R=gas constant = 0.0821 atm.L/K.mol
W= 2.2 x 0.0821 x 490 ln2 atm.L
W=61.34 atm.L
W=Q= 61.34 atm.L
We know that
1 atm.L = 101.3 J
Q= 6213.72 J
