First Law of Thermodynamics Past Year (2019 onward - NTA Papers) MCQs Thermodynamics Chemistry NEET Practice Questions, MCQs, Past Year Questions (PYQs), NCERT Questions, Question Bank, Class 11 and Class 12 Questions, and PDF solved with answers

The work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from pressure of 20 atmosphere to 10 atmosphere is :
( Given R = 2.0 cal K^-1 mol^-1)

1. -413.14 calories
2. 413.14 calories
3. 100 calories
4. 0 calorie

Subtopic: First Law of Thermodynamics |

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Choose the correct statement for the work done in the expansion and heat absorbed or released when 5 liters of an ideal gas at 10 atmospheric pressure isothermally expands into a vacuum until the volume is 15 liters:

1.	Both the heat and work done will be greater than zero.
2.	Heat absorbed will be less than zero and work done will be positive.
3.	Work done will be zero and heat will also be zero.
4.	Work done will be greater than zero and heat will remain zero.

Subtopic: First Law of Thermodynamics |

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The work done when 1 mole of gas expands reversibly and isothermally from a pressure of 5 atm to 1 atm at 300 K is:
(Given log 5 = 0.6989 and R = 8.314 J K^-1 mol^-1)
1. zero J
2. 150 J
3. +4014.6 J
4. -4014.6 J

Subtopic: First Law of Thermodynamics |

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One mole of an ideal gas at 300 K is expanded isothermally from 1 L to 10 L volume. $\Delta U$ for this process is:
(Use R = 8.314 J K^–1 mol^–1)

1.	1260 J	2.	2520 J
3.	5040 J	4.	0 J

Subtopic: First Law of Thermodynamics |

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An ideal gas expands isothermally from $10^{- 3} m^{3} t o 10^{- 2} m^{3}$ at 300 K against a constant pressure of $10^{5} N m^{- 2}$ . The work done by the gas is:

1.	+270 kJ	2.	–900 J
3.	+900 kJ	4.	–900 kJ

Subtopic: First Law of Thermodynamics |

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