Question

Calculate the total expansion work done by 1.00 mol ideal gas in a process that follows the path (1>2>3>4>5>6) as indicated in the following diagram.

Top Figure: What is the temperate of the gas at the isothermal curve in the diagram?

Bottom Figure: The cartoon below represents an experimental setup for conducting the process in the diagram above. What would you have to do to achieve step 1>2 if the cartoon shows the conditions at 1?

Chegg won't let me upload the image clearly so here is the figure: http://postimg.org/image/k69x0gbrt/

Answer 1

a sthe graph indicate a reversible process , we knoew that work done is a path function hence total work done is some of all individual work done

W = -p(V_{2 -}V₁) = -24 * (3-1) = 48 * 101.3 =4862.4 j 1 L atm = 101.3 joules

W= - 2.303 nRT log V₁/V₂= -2.303 * 1 * 8.314 * T log 1/8

4862.4    /-2.303 * 1 * 8.314   log 8/1 = T

t = 281.21 K

What would you have to do to achieve step if the cartoon shows the conditions at 1

we must lower the external pressure by removing thye bricks from the piston .