The decrease in available energy is calculated using the formula:
\( \Delta Q = \dot{Q} \left( 1 - \frac{T_2}{T_1} \right) \)
Where: \( \dot{Q} = 7200 \, \text{kJ/min}, \, T_1 = 1000 \, K, \, \text{and} \, T_2 = 300 \, K \). After plugging in the values:
\( \Delta Q = 7200 \times \left( 1 - \frac{300}{1000} \right) = 7200 \times 0.7 = 5040 \, \text{kJ/min} \)
A closed system is undergoing a reversible process 1–P–2 from state 1 to 2, as shown in the figure, where X and Y are thermodynamic properties. An irreversible process 2–Q–1 brings the system back from 2 to 1. The net change in entropy of the system and surroundings during the above-mentioned cycle are _______ respectively.
Consider a weightless, frictionless piston with a 2 kg mass placed on it as shown in the figure. At equilibrium in position 1, the cylinder contains 0.1 kg of air. The piston cross-sectional area is 0.01 m2. The ambient pressure in the surroundings outside the piston-cylinder arrangement is 0 bar (absolute). When the mass above the piston is removed instantaneously, it moves up and hits the stop at position 2, which is 0.1 m above the initial position.
Assuming \( g = 9.81 \, {m/s}^2 \), the thermodynamic work done by the system during this process is ________ J (answer in integer).
An ideal gas has undergone through the cyclic process as shown in the figure. Work done by the gas in the entire cycle is _____ $ \times 10^{-1} $ J. (Take $ \pi = 3.14 $)