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qUESTIONS

A cyclic process ABCA is shown in V-T diagram (Fig (a)). It is performed with a constant mass of ideal gas. How will this transform to a p-V digram?

Cyclic process: The total work done in the cyclic process shown in the Fig. 4.19 is -1000 J. (a) What does the negative sign mean? (b) What is the change in internal energy and the heat transferred during this process. (c) What will happen when the direction of the cycle is changed?

An ideal gas of volume 1.0L is adiabatically compressed to (1/15)th of its initial volume. Its initial pressure and temperature is 1.01 ×105 Pa and 27°C respectively. Given C for ideal gas 20.8J/mol.K and y = 1.4. Calculate (a) final pressure, (b) work done, and (c) final temperature. (d) How would your answers change, if the process were isothermal?

One mole of an ideal gas is initially kept in a cylinder with a movable frictionless and massless piston at pressure of 1.0mPa, and temperature 27°C. It is then expanded till its volume is doubled. How much work is done if the expansion is isobaric?

0.5 mole of gas at temp 300 K expands isothermally from an initial volume of 2.0L to final volume of 6.0L. (a) What is the work done by the gas? (R = 8.31 J mol-¹ K-‘), (b) How much heat is supplied to the gas?

104 kJ of work is done on certain volume of a gas. If the gas releases 125 kJ of heat, calculate the change in internal energy (in kJ) of the gas.

1.0 kg of liquid water is boiled at 100 °C and all of it is converted to steam. If the change of state takes place at the atmospheric pressure (1.01×10^5 Pa), calculate (a) the energy transferred to the system, (b) the work done by the system during this change, and (c) the change in the internal energy of the system. Given, the volume of water changes from 1.0 x 10³ m³ in liquid form to 1.671 m³ when in the form of steam.

A gas enclosed in a cylinder is expanded to double its initial volume at a constant pressure of one atmosphere. How much work is done in this process?

Calculate the internal energy of argon and oxygen.

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