Suppose 2.00 mol of a diatomic gas is taken reversibly around the cycle shown in the T-S diagram of figure, where S 1 = 6.00 J / K and S 2 = 8.00 J / K . The molecules do not rotate or oscillate.

Question

Suppose 2.00 mol of a diatomic gas is taken reversibly around the cycle shown in the T-S diagram of figure, where $S_{1} = 6.00 J / K$ and $S_{2} = 8.00 J / K$ . The molecules do not rotate or oscillate. What is the energy transferred as heat Q for (a) path $1 \to 2$ , (b) the full cycle? The volume $V_{1}$ in state 1 is $0.200 m^{2}$ , What is the volume in (c) state 2 and (d) state 3 ?

TestHub · Accepted Answer

Q 12 ​ = 350 × 2 = 700 J ​ Q 23 ​ = 0 Q C yc l e ​ = 2 1 ​ × 2 × 50 = 50 J W 12 ​ = Q 12 ​ = 700 J Q 12 ​ = Δ U + W = n RT ℓ n ( V 1 ​ V 2 ​ ​ ) 700 = 2 × 3 25 ​ × 350 ℓ n 0.2 V 2 ​ ​ 0.2 V 2 ​ ​ = e 1/25 = 1.04 V 2 ​ = 0.208 m 3 T 2 ​ V 2 γ − 1 ​ = T 3 ​ V 3 γ − 1 ​ 300 350 × 0.208 ​ ​ = V 3 ​ ​ V 3 ​ = 36 49 ​ × 0.208 = 0.283 m 3 ​

Physics - Heat & Thermo Question with Solution | TestHub

Options:(select one or more)

Doubts & Discussion