Question

n moles of CO2 gas (T1, V1) obey a van der Waals equation of state are contained in an insulated piston-cylinder arrangement. A reversible expansion of the gas is carried out until the volume become 2V1.
[CV.m = 28.80 J mol−1K−1, a = 3.610 atm. dm6. mol−2, b = 4.29 x 10−2 dm3. mol−1]
(a) Find the final temperature of gas as a function of n, . , T1, V1 and the van
der Waals parameter a and b.
(b) If two moles of CO2 gas involved and T1 = 350K, V1 = 40L, compute final
temperature of the gas.
(c) Find work done and internal energy of the gas.

Answer 1

Answer:

one or two three or four

Explanation:

animals of CO2 gas find the final temperature of gas

Answer 2

The final temperature of the 2 moles of gas has been 0.0014 K.

The gas has been assumed to be the ideal gas. The moles of the has been n. According to the ideal gas equation:

(a) PV= nRT.

For the reversible expansion of 1 mole of gas:

P = $\rm \dfrac{RT}{V - b}\;\times\;\dfrac{a}{V^2}$

For n moles of gas, the reversible expansion will be:

P = $\rm \dfrac{nRT}{V - b}\;\times\;\dfrac{a}{V^2}$

The final temperature of the reversible expansion has been:

$\rm T_f\;=\;T_i\;+\;\dfrac{an^2\;[\frac{1}{Vf\;-\;\frac{1}{Vi} } ]}{Cv}$

(B) The ideal gas equation can be given as:

$\rm \dfrac{P1V1}{nT1}\;=\; \dfrac{P2V2}{nT2}$

Substituting the values:

$\rm \dfrac{40}{2\;\times\;350}\;=\;\dfrac{80}{2\;\times\;T2}$

T2 = 0.0014 K.

The final temperature of the 2 moles of gas has been 0.0014 K.

(c) The work done can be given by:

W = nRT In$\rm \dfrac{V2}{V1}$

The internal energy of the system has been given by:

$\Delta$U = $\rm C_v$[$\rm T_f\;-\;T_i$] - a$\rm n^2$ $\rm [\dfrac{1}{Vf}\;-\;\dfrac{1}{Vi} ]$

For more information about the reversible expansion of gas, refer to the link:

https://brainly.com/question/22791115