Calculate moles O_{2} produced using the ideal gas equation:

$\overline{)\mathbf{PV}\mathbf{=}\mathbf{nRT}}$

$\mathbf{P}\mathbf{=}\mathbf{746}\mathbf{}\overline{)\mathbf{mmHg}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{atm}}{\mathbf{760}\mathbf{}\overline{)\mathbf{mmHg}}}$

P = 0.9815 atm

V = 4.55 L

T = 308 K

$\frac{\mathbf{PV}}{\mathbf{RT}}\mathbf{=}\frac{\mathbf{n}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\mathbf{n}\mathbf{=}\frac{\mathbf{PV}}{\mathbf{RT}}\phantom{\rule{0ex}{0ex}}\mathbf{n}\mathbf{=}\frac{(0.9815\overline{)\mathrm{atm}})(4.55\overline{)L})}{(0.08206{\displaystyle \frac{\overline{)L}\xb7\overline{)\mathrm{atm}}}{\mathrm{mol}\xb7\overline{)K}}})(308\overline{)K})}$

In the reaction shown here, 4.55 L of O_{2} was formed at P = 746 mmHg and T = 308 K .

2Ag_{2}O(s) → 4Ag(s)+O_{2}(g)

How many grams of Ag_{2}O decomposed?

Frequently Asked Questions

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 Gas Stoichiometry concept. If you need more Gas Stoichiometry practice, you can also practice Gas Stoichiometry practice problems.