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Temperature

why is it so ...

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why is it so that if volume remains constant then work done is taken zero?

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Q. 0.5 mole of diatomic gas at

27^{0} C

is heated at constant pressure so that its volume is trebled. If

R = 8.3 J m o l e^{- 1} k^{- 1}

then work done is

1 g $H_{2}$ gas as STP is expanded so that volume is doubled. Hence, work done is

Q. 0.1 moles of a diatomic gas at

27^{0} C

is heated at constant pressure, so that the volume is doubled. If

R = 2

cal/mol, the work done is :

1 g H_{2}

gas STP is expanded so that the volume is doubled. Hence, work done is

30 k c a l

is supplied to a system and

4200 J

of external work is done on the system so that its volume decreases at constant pressure. What is the change in its internal energy.

= (J = 4200 J / k c a l)

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