# Problem: One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T= 300 K: 1 L•atm = 101.3 J) A. 375 J B. 751 J C. 225 x 103 J D. 852 J E. none of these

###### FREE Expert Solution

We’re being asked to calculate the work for the system if 1 mole of ideal gas expanded from a volume of 1.00 L to a volume of 8.41 L against a constant external pressure of 1.00 atm.

Recall that work (w) is given by:

$\overline{){\mathbf{w}}{\mathbf{=}}{\mathbf{-}}{\mathbf{P\Delta V}}}$

where:

P = pressure (in atm)

ΔV = Vfinal – Vinitial = change in volume (in L)

Also note that if work is:

• (+): work is done by the surroundings to the system (compression)

• (–): work is done by the system to the surroundings (expansion) ###### Problem Details

One mole of an ideal gas is expanded from a volume of 1.00 liter to a volume of 8.41 liters against a constant external pressure of 1.00 atm. How much work (in joules) is performed on the surroundings? Ignore significant figures for this problem. (T= 300 K: 1 L•atm = 101.3 J)

A. 375 J

B. 751 J

C. 225 x 103

D. 852 J

E. none of these

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