# 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

🤓 Based on our data, we think this question is relevant for Professor Smith's class at UH.

###### 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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Internal Energy concept. You can view video lessons to learn Internal Energy. Or if you need more Internal Energy practice, you can also practice Internal Energy practice problems.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Smith's class at UH.