MediumChemistryHigh School (11–12)Chemical Thermodynamics › Systems, Work, Heat and the First LawNumericalpython

2.00 mol of an ideal gas at 310 K expands reversibly and at constant temperature from 5.00 L to…

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

$2.00$ mol of an ideal gas at $310$ K expands reversibly and at constant temperature from $5.00$ L to $20.0$ L. Find $w$ , $\Delta U$ and $q$ , in kJ. Use $R = 8.314$ 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

← 0.80 mol of an ideal gas expands at constant temperature from 4.0 L into an evacuated vessel, until…1.00 mol of an ideal gas at 300 K expands at constant temperature from 10.0 bar to 2.00 bar. →

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

Discussion (0)

Loading…

2.00 mol of an ideal gas at 310 K expands reversibly and at constant temperature from 5.00 L to…

The worked solution

Discussion (0)

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