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

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** = V_{final} – V_{initial} = 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)*

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 10^{3} J

D. 852 J

E. none of these

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