Question

Many compressed gases come in large metal cylinders. An 80.0 tank of nitrogen gas pressurized to 172 is left in the sun and heats from its normal temperature of 20.0 °C to 140.0 °C. Assume that the nitrogen gas behaves ideally and that the molar constant-volume heat capacity of diatomic nitrogen is 21.0. (a) Calculate the number of moles of gas in the tank. (b) Calculate the final pressure inside the tank. (c) Calculate the work, of the process. (d) Calculate the heat, of the process. (e) Calculate the change in internal energy, Δ, of the process.

Answer 1

Answer:

We have, Volume of cylinder, V = 80 L Pressure of the gas, P = 172 atm (Initially) Temperature, T =20.0°C = 293 K According to the Ideal Gas Law, PV = nRT 172 * 80 = n * 0.082 * 293 n = 572.71 moles (a) Final temperature = 140.0°C Final Pressure,P = ? Volume, V = 80 L (Volume of such cylinders remain the same) PV = nRT P * 80= 572.71 * 0.082 * 413 P = 242.44 atm (b) Since the final volume and...

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Explanation:

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