Ozzie wanted to do another experiment with a stronger h₂o₂ solution to check the accuracy of the experiment by calculating the theoretical volume of o₂(g) it would produce. then he could compare his experimental volume of o₂(g) to the theoretical volume of o₂(g). he used 4.20 ml of 2.57 m h₂o₂ and the partial pressure of o₂ was 0.9624 atm and the temperature was 300.95 k. what volume of o₂(g) could he theoretically produce (in ml)?

Explanation:

Reaction for decomposition of is as follows.

Molarity of = 2.57 M

Volume = 4.20 ml

             =

             = 0.0042 L

Now, calculate the moles of as follows.

             Moles of = Molarity × Volume

                                           =

                                           = 0.0107 mol

According to the balanced equation, 2 mole of gives 1 mole of .

Hence, 0.0107 mol of gives 0.00575 mol of .

Partial pressure of = 0.9624 atm

Temperature = 300.95 K

Now, using ideal gas equation we will calculate the volume as follows.

                              PV = nRT

                         V =

                            =

                             = 0.1475 L

or,                          = 147.5 ml               (as 1 L = 1000 mL)

Thus, we can conclude that volume of is 147.5 ml.

explanation:

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