First Law of Thermodynamics
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CHXI06:THERMODYNAMICS

369377 A gas expands isothermally and reversibly. The work done by the gas is

1 Zero
2 Maximum
3 Minimum
4 Cannot be determined
CHXI06:THERMODYNAMICS

369378 The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at \(\mathrm{25^{\circ} \mathrm{C}}\) is

1 \(\mathrm{-2.303 \times 298 \times 0.082 \log 2}\)
2 \(\mathrm{-298 \times 10^{7} \times 8.31 \times 2.303 \log 2}\)
3 \(\mathrm{2.303 \times 298 \times 0.082 \log 0.5}\)
4 \(\mathrm{2.303 \times 298 \times 2 \log 2}\).
CHXI06:THERMODYNAMICS

369379 If 1 mole of an ideal gas expands isothermally at \(37^{\circ} \mathrm{C}\) from \(15 \mathrm{~L}\) to \(25 \mathrm{~L}\), the maximum work obtained is

1 \(12.87 \mathrm{~J}\)
2 \(6.43 \mathrm{~J}\)
3 \(8.57 \mathrm{~J}\)
4 \(2.92 \mathrm{~J}\)
CHXI06:THERMODYNAMICS

369380 1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure from \(210 \mathrm{kPa}\) to \(105 \mathrm{kPa}\) at \(300 \mathrm{~K}\). What is the work done? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

1 \(1960 \mathrm{~J}\)
2 \(864 \mathrm{~J}\)
3 \(1296 \mathrm{~J}\)
4 \(1729 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS

369381 For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression, \(\mathrm{\mathrm{w}=-n \mathrm{RT} \ln \dfrac{\mathrm{V}_{\mathrm{f}}}{\mathrm{V}_{\mathrm{i}}}}\). A sample containing \(\mathrm{1.0 \mathrm{~mol}}\) of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at \(\mathrm{300 \mathrm{~K}}\) and at \(\mathrm{600 \mathrm{~K}}\) respectively. Choose the correct option.

1 Work done at \(\mathrm{600 \mathrm{~K}}\) is 20 times the work done at \(\mathrm{300 \mathrm{~K}}\).
2 Work done at \(\mathrm{300 \mathrm{~K}}\) is twice the work done at \(\mathrm{600 \mathrm{~K}}\).
3 Work done at \(\mathrm{600 \mathrm{~K}}\) is twice the work done at \(\mathrm{300 \mathrm{~K}}\).
4 \(\mathrm{\Delta \mathrm{U}=0}\) in only one case.
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CHXI06:THERMODYNAMICS

369377 A gas expands isothermally and reversibly. The work done by the gas is

1 Zero
2 Maximum
3 Minimum
4 Cannot be determined
CHXI06:THERMODYNAMICS

369378 The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at \(\mathrm{25^{\circ} \mathrm{C}}\) is

1 \(\mathrm{-2.303 \times 298 \times 0.082 \log 2}\)
2 \(\mathrm{-298 \times 10^{7} \times 8.31 \times 2.303 \log 2}\)
3 \(\mathrm{2.303 \times 298 \times 0.082 \log 0.5}\)
4 \(\mathrm{2.303 \times 298 \times 2 \log 2}\).
CHXI06:THERMODYNAMICS

369379 If 1 mole of an ideal gas expands isothermally at \(37^{\circ} \mathrm{C}\) from \(15 \mathrm{~L}\) to \(25 \mathrm{~L}\), the maximum work obtained is

1 \(12.87 \mathrm{~J}\)
2 \(6.43 \mathrm{~J}\)
3 \(8.57 \mathrm{~J}\)
4 \(2.92 \mathrm{~J}\)
CHXI06:THERMODYNAMICS

369380 1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure from \(210 \mathrm{kPa}\) to \(105 \mathrm{kPa}\) at \(300 \mathrm{~K}\). What is the work done? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

1 \(1960 \mathrm{~J}\)
2 \(864 \mathrm{~J}\)
3 \(1296 \mathrm{~J}\)
4 \(1729 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS

369381 For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression, \(\mathrm{\mathrm{w}=-n \mathrm{RT} \ln \dfrac{\mathrm{V}_{\mathrm{f}}}{\mathrm{V}_{\mathrm{i}}}}\). A sample containing \(\mathrm{1.0 \mathrm{~mol}}\) of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at \(\mathrm{300 \mathrm{~K}}\) and at \(\mathrm{600 \mathrm{~K}}\) respectively. Choose the correct option.

1 Work done at \(\mathrm{600 \mathrm{~K}}\) is 20 times the work done at \(\mathrm{300 \mathrm{~K}}\).
2 Work done at \(\mathrm{300 \mathrm{~K}}\) is twice the work done at \(\mathrm{600 \mathrm{~K}}\).
3 Work done at \(\mathrm{600 \mathrm{~K}}\) is twice the work done at \(\mathrm{300 \mathrm{~K}}\).
4 \(\mathrm{\Delta \mathrm{U}=0}\) in only one case.
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CHXI06:THERMODYNAMICS

369377 A gas expands isothermally and reversibly. The work done by the gas is

1 Zero
2 Maximum
3 Minimum
4 Cannot be determined
CHXI06:THERMODYNAMICS

369378 The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at \(\mathrm{25^{\circ} \mathrm{C}}\) is

1 \(\mathrm{-2.303 \times 298 \times 0.082 \log 2}\)
2 \(\mathrm{-298 \times 10^{7} \times 8.31 \times 2.303 \log 2}\)
3 \(\mathrm{2.303 \times 298 \times 0.082 \log 0.5}\)
4 \(\mathrm{2.303 \times 298 \times 2 \log 2}\).
CHXI06:THERMODYNAMICS

369379 If 1 mole of an ideal gas expands isothermally at \(37^{\circ} \mathrm{C}\) from \(15 \mathrm{~L}\) to \(25 \mathrm{~L}\), the maximum work obtained is

1 \(12.87 \mathrm{~J}\)
2 \(6.43 \mathrm{~J}\)
3 \(8.57 \mathrm{~J}\)
4 \(2.92 \mathrm{~J}\)
CHXI06:THERMODYNAMICS

369380 1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure from \(210 \mathrm{kPa}\) to \(105 \mathrm{kPa}\) at \(300 \mathrm{~K}\). What is the work done? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

1 \(1960 \mathrm{~J}\)
2 \(864 \mathrm{~J}\)
3 \(1296 \mathrm{~J}\)
4 \(1729 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS

369381 For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression, \(\mathrm{\mathrm{w}=-n \mathrm{RT} \ln \dfrac{\mathrm{V}_{\mathrm{f}}}{\mathrm{V}_{\mathrm{i}}}}\). A sample containing \(\mathrm{1.0 \mathrm{~mol}}\) of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at \(\mathrm{300 \mathrm{~K}}\) and at \(\mathrm{600 \mathrm{~K}}\) respectively. Choose the correct option.

1 Work done at \(\mathrm{600 \mathrm{~K}}\) is 20 times the work done at \(\mathrm{300 \mathrm{~K}}\).
2 Work done at \(\mathrm{300 \mathrm{~K}}\) is twice the work done at \(\mathrm{600 \mathrm{~K}}\).
3 Work done at \(\mathrm{600 \mathrm{~K}}\) is twice the work done at \(\mathrm{300 \mathrm{~K}}\).
4 \(\mathrm{\Delta \mathrm{U}=0}\) in only one case.
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CHXI06:THERMODYNAMICS

369377 A gas expands isothermally and reversibly. The work done by the gas is

1 Zero
2 Maximum
3 Minimum
4 Cannot be determined
CHXI06:THERMODYNAMICS

369378 The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at \(\mathrm{25^{\circ} \mathrm{C}}\) is

1 \(\mathrm{-2.303 \times 298 \times 0.082 \log 2}\)
2 \(\mathrm{-298 \times 10^{7} \times 8.31 \times 2.303 \log 2}\)
3 \(\mathrm{2.303 \times 298 \times 0.082 \log 0.5}\)
4 \(\mathrm{2.303 \times 298 \times 2 \log 2}\).
CHXI06:THERMODYNAMICS

369379 If 1 mole of an ideal gas expands isothermally at \(37^{\circ} \mathrm{C}\) from \(15 \mathrm{~L}\) to \(25 \mathrm{~L}\), the maximum work obtained is

1 \(12.87 \mathrm{~J}\)
2 \(6.43 \mathrm{~J}\)
3 \(8.57 \mathrm{~J}\)
4 \(2.92 \mathrm{~J}\)
CHXI06:THERMODYNAMICS

369380 1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure from \(210 \mathrm{kPa}\) to \(105 \mathrm{kPa}\) at \(300 \mathrm{~K}\). What is the work done? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

1 \(1960 \mathrm{~J}\)
2 \(864 \mathrm{~J}\)
3 \(1296 \mathrm{~J}\)
4 \(1729 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS

369381 For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression, \(\mathrm{\mathrm{w}=-n \mathrm{RT} \ln \dfrac{\mathrm{V}_{\mathrm{f}}}{\mathrm{V}_{\mathrm{i}}}}\). A sample containing \(\mathrm{1.0 \mathrm{~mol}}\) of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at \(\mathrm{300 \mathrm{~K}}\) and at \(\mathrm{600 \mathrm{~K}}\) respectively. Choose the correct option.

1 Work done at \(\mathrm{600 \mathrm{~K}}\) is 20 times the work done at \(\mathrm{300 \mathrm{~K}}\).
2 Work done at \(\mathrm{300 \mathrm{~K}}\) is twice the work done at \(\mathrm{600 \mathrm{~K}}\).
3 Work done at \(\mathrm{600 \mathrm{~K}}\) is twice the work done at \(\mathrm{300 \mathrm{~K}}\).
4 \(\mathrm{\Delta \mathrm{U}=0}\) in only one case.
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CHXI06:THERMODYNAMICS

369377 A gas expands isothermally and reversibly. The work done by the gas is

1 Zero
2 Maximum
3 Minimum
4 Cannot be determined
CHXI06:THERMODYNAMICS

369378 The work done in ergs for the reversible expansion of one mole of an ideal gas from a volume of 10 litres to 20 litres at \(\mathrm{25^{\circ} \mathrm{C}}\) is

1 \(\mathrm{-2.303 \times 298 \times 0.082 \log 2}\)
2 \(\mathrm{-298 \times 10^{7} \times 8.31 \times 2.303 \log 2}\)
3 \(\mathrm{2.303 \times 298 \times 0.082 \log 0.5}\)
4 \(\mathrm{2.303 \times 298 \times 2 \log 2}\).
CHXI06:THERMODYNAMICS

369379 If 1 mole of an ideal gas expands isothermally at \(37^{\circ} \mathrm{C}\) from \(15 \mathrm{~L}\) to \(25 \mathrm{~L}\), the maximum work obtained is

1 \(12.87 \mathrm{~J}\)
2 \(6.43 \mathrm{~J}\)
3 \(8.57 \mathrm{~J}\)
4 \(2.92 \mathrm{~J}\)
CHXI06:THERMODYNAMICS

369380 1 mole of an ideal gas expands isothermally and reversibly by decreasing pressure from \(210 \mathrm{kPa}\) to \(105 \mathrm{kPa}\) at \(300 \mathrm{~K}\). What is the work done? \(\left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}\right)\)

1 \(1960 \mathrm{~J}\)
2 \(864 \mathrm{~J}\)
3 \(1296 \mathrm{~J}\)
4 \(1729 \mathrm{~J}\)
MHTCET - 2021
CHXI06:THERMODYNAMICS

369381 For an ideal gas, the work of reversible expansion under isothermal condition can be calculated by using the expression, \(\mathrm{\mathrm{w}=-n \mathrm{RT} \ln \dfrac{\mathrm{V}_{\mathrm{f}}}{\mathrm{V}_{\mathrm{i}}}}\). A sample containing \(\mathrm{1.0 \mathrm{~mol}}\) of an ideal gas is expanded isothermally and reversibly to ten times of its original volume, in two separate experiments. The expansion is carried out at \(\mathrm{300 \mathrm{~K}}\) and at \(\mathrm{600 \mathrm{~K}}\) respectively. Choose the correct option.

1 Work done at \(\mathrm{600 \mathrm{~K}}\) is 20 times the work done at \(\mathrm{300 \mathrm{~K}}\).
2 Work done at \(\mathrm{300 \mathrm{~K}}\) is twice the work done at \(\mathrm{600 \mathrm{~K}}\).
3 Work done at \(\mathrm{600 \mathrm{~K}}\) is twice the work done at \(\mathrm{300 \mathrm{~K}}\).
4 \(\mathrm{\Delta \mathrm{U}=0}\) in only one case.