HardChemistryHigh School (11–12)Chemical Thermodynamics › Systems, Work, Heat and the First LawNumericalpythonNEET Board Exam

1.00 mol of an ideal gas at 300 K expands at constant temperature from 10.0 bar to 2.00 bar…

Contributed by StemPy Lab

Try it on paper first. A hint, the key idea and the worked solution are here when you need them.

$1.00$ mol of an ideal gas at $300$ K expands at constant temperature from $10.0$ bar to $2.00$ bar. Find its starting and final volumes. Then find the work (a) in one step against a constant outside pressure of $2.00$ bar, and (b) reversibly. Use $R = 0.08314$ L bar K $^{-1}$ mol $^{-1}$ $= 8.314$ J K $^{-1}$ mol $^{-1}$ .

Need a reminder? The key ideaShow

Work against a constant outside pressure: $w = -p_\text{ex}\Delta V$ , with $1$ L bar $= 100$ J and $1$ L atm $= 101.3$ J. Free expansion: $w = 0$ . Reversible isothermal ideal gas: $w = -2.303\,nRT\log\dfrac{V_f}{V_i}$ , and $\Delta U = 0$ , so $q = -w$ .

The worked solution

Have you tried it?

Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.

← All Problems

← 2.00 mol of an ideal gas at 310 K expands reversibly and at constant temperature from 5.00 L to…50.0 mL of 1.00 M hydrochloric acid is mixed with 50.0 mL of 1.00 M sodium hydroxide in a… →

More onChemical Thermodynamics › Systems, Work, Heat and the First Law

Discussion (0)

Loading…

1.00 mol of an ideal gas at 300 K expands at constant temperature from 10.0 bar to 2.00 bar…

The worked solution

Discussion (0)

Want to go further in Chemical Thermodynamics › Systems, Work, Heat and the First Law?