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A reaction taking place in a container with a piston-cylinder assembly at constant temperature produces a gas, and the volume increases from 127 mL to 654 mL against an external pressure of 860 torr. Calculate the work done in Joules (J)

Respuesta :

skyluke89

Answer:

60.4 J

Explanation:

The work done by the gas is given by:

[tex]W=p(V_f-V_i)[/tex]

where

p is the gas pressure

[tex]V_f[/tex] is the final volume of the gas

[tex]V_i[/tex] is the initial volume

We must convert all the quantities into SI units:

[tex]p=860 torr \cdot \frac{1.013\cdot 10^5 pa}{760 torr}=1.146\cdot 10^5 Pa[/tex]

[tex]V_i = 127 mL = 0.127 L = 0.127 dm^3 = 0.127 \cdot 10^{-3}m^2[/tex]

[tex]V_f = 654 mL = 0.654 L = 0.654 dm^3 = 0.654 \cdot 10^{-3}m^2[/tex]

So the work done is

[tex]W=(1.146\cdot 10^5 Pa)(0.654\cdot 10^{-3} m^3-0.127\cdot 10^{-3} m^3)=60.4 J[/tex]

zainsubhani

Answer:

[tex]W=60.4 J[/tex]

Work done is 60.4 Joules (J)

Explanation:

Work done 'W' is given by:

[tex]W=P\triangle V[/tex]

Where:

ΔV is the change in Volume.

P is the pressure.

Change in Volume=Final Volume-Initial Volume

Initial Volume= 127 mL

Final Volume= 654 mL

ΔV=654-127 (mL)

ΔV=527 mL

ΔV=0.527 L

Pressure Conversion:

1 atm=760 torr

[tex]P=\frac{860}{760} \\P=1.1315\ atm[/tex]

Now,

[tex]W=P\triangle V[/tex]

[tex]W=1.1315\ atm*0.527\ L[/tex]

[tex]W=0.5963 L.atm[/tex]

In joule (J): (Conversion 1 atm. L=101.325 J)

[tex]W=0.5963\ L.atm*\frac{101.325 J}{1\ L.atm}[/tex]

[tex]W=60.4 J[/tex]

Work done is 60.4 Joules (J)

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