A piston filled with 0.04 mol of an ideal gas expands reversibly form 50.0 mL to 375 mL at a constant temperature of ${37.0}^{o} C$ . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be:
(R = 8.314 J/mol K) (ln 7.5 = 2.01)

q = -208 J, w = -208 J

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q = -208 J, w = +208 J

No worries! We‘ve got your back. Try BYJU‘S free classes today!

q = +208 J, w = +208 J

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q = +208 J, w = -208 J

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Solution

The correct option is D q = +208 J, w = -208 J
Process is isothermal reversible expansion, hence $△ U = 0.$
$∴$ q = -w As q = +208 J Hence, w = -208 J

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Similar questions

Q. A piston filled with 0.04 mol of an ideal gas expands reversibly form 50.0 mL to 375 mL at a constant temperature of

{37.0}^{o} C

. As it does so, it absorbs 208 J of heat. The values of q and w for the process will be:
(R = 8.314 J/mol K) (ln 7.5 = 2.01)

A piston filled with 0.04 mole of an ideal gas expands reversibly from 50.0 L to 375 mL at a constant temperature of ${37.0}^{\circ} C$ . As it does so, it absorbs 208 J of heat energy. The values of q and W for the process will be (R = 8.314 J/mol K, ln 7.5 = 2.01)

Q. A piston filled with 0.04 mole of an ideal gas expand reversibly from 50.0mL to 375 mL at a consumed temperature of

{37.0}^{\circ} C

. As it does so, it absorbs

208^{\circ} C

heat. The values of q and W for the process will be
(R = 8.314J/mol K, In 7.5 = 2.01)

Q. A piston filled with 0.04 moles of an ideal gas expands reversibly from 50.0 L to 375.0 L at a constant temperature of

{37.0}^{\circ} C

. As it does so, it absorbs 208 J of heat energy. The value of work done (in

J

) for the process will be: (R = 8.314 J/mol K, ln 7.5 = 2.01)

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A piston filled with 0.04 mol of an ideal gas expands reversibly form 50.0 mL to 375 mL at a constant temperature of 37.0oC. As it does so, it absorbs 208 J of heat. The values of q and w for the process will be: (R = 8.314 J/mol K) (ln 7.5 = 2.01)

The correct option is D q = +208 J, w = -208 J Process is isothermal reversible expansion, hence △U=0. ∴ q = -w As q = +208 J Hence, w = -208 J

A piston filled with 0.04 mol of an ideal gas expands reversibly form 50.0 mL to 375 mL at a constant temperature of ${37.0}^{o} C$ . As it does so, it absorbs 208 J of heat. The values of q and w for the process will be:
(R = 8.314 J/mol K) (ln 7.5 = 2.01)

The correct option is D q = +208 J, w = -208 J
Process is isothermal reversible expansion, hence $△ U = 0.$
$∴$ q = -w As q = +208 J Hence, w = -208 J