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- 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 7-5-2-01A- q-208 J - W -208 JB- q-208 J - W -208 JC- q-208 J - W-208 JD- q-208 J - W -208 J

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Standard XII

Chemistry

Thermodynamic Processes

A piston fill...

Question

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 = + 208 J, W = - 208 J

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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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Solution

The correct option is A q = + 208 J, W = - 208 J
The process is isothermal expansion, hence
q = - W
$Δ E = 0$
$W = - 2.303 n R T l o g \frac{V_{2}}{V_{1}}$
$= - 2.303 \times 0.04 \times 8.314 \times 310 \times l o g \frac{335}{50}$
$= - 208 J$
q = + 208 J, W = -208 J (expansion work)

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Similar questions

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

mol of an ideal gas expands reversibly from

50.0 m L

375 m L

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 / m o l

K

) (

ln 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)

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

moles of an ideal gas expands reversibly from

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. What will be the value of

q

and

W

respectively ?

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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∘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)

The correct option is A q = + 208 J, W = - 208 J The process is isothermal expansion, hence q = - W ΔE=0 W=−2.303nRTlogV2V1 =−2.303×0.04×8.314×310×log33550 =−208 J q = + 208 J, W = -208 J (expansion work)

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)

The correct option is A q = + 208 J, W = - 208 J
The process is isothermal expansion, hence
q = - W
$Δ E = 0$
$W = - 2.303 n R T l o g \frac{V_{2}}{V_{1}}$
$= - 2.303 \times 0.04 \times 8.314 \times 310 \times l o g \frac{335}{50}$
$= - 208 J$
q = + 208 J, W = -208 J (expansion work)