If 2.18 g of sodium peroxide (Na2O2) react with water to produce sodium hydroxide abs oxygen, how many liters of oxygen will be produced at 17.7 Celsius abs 726 torr?

0.350 L

Explanation:

First we convert 2.18 g of Na₂O₂ into moles, using its molar mass:

Then we convert 0.0279 moles of Na₂O₂ into moles of O₂, using the stoichiometric coefficients of the reaction:

Finally we use the PV=nRT formula to calculate the volume of oxygen produced:

Inputting the data:

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole