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marin [14]
3 years ago
8

A container of gas is at a pressure of 1.3 x 10^5 pa and a volume of 6.0 m^3. how much work is done by the gas if it expands at

a constant pressure to twice its initial volume
Chemistry
2 answers:
Amanda [17]3 years ago
8 0

<u>Answer:</u> The work done for the given process is -778 kJ

<u>Explanation:</u>

To calculate the amount of work done for an isothermal process is given by the equation:

W=-P\Delta V=-P(V_2-V_1)

W = amount of work done = ?

P = pressure of the container = 1.3\times 10^5Pa=1.28atm    (Conversion factor:  1atm=1.013\times 10^5Pa  )

V_1 = initial volume = 6.0m^3=6000L     (Conversion factor:  1m^3=1000L  )

V_2 = final volume = (2\times V_1)=(2\times 6000)=12000L

Putting values in above equation, we get:

W=-1.28atm\times (12000-6000)L=-7680L.atm

To convert this into joules, we use the conversion factor:

1L.atm=101.33J

1 kJ = 1000 J

So, -7680L.atm=-35\times 101.3=-777984J=-778kJ

The negative sign indicates the system is doing work.

Hence, the work done for the given process is -778 kJ

kozerog [31]3 years ago
5 0
For the answer to the question above, since the process is carried out at constant pressure, 
<span>work = P (V1-V2) </span>
<span>= 1.3 E5 (6-12) = -7.8 E5 N.m (in this case the work is made by the system, so it is negative if work made on the system then it should be positive)</span>
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