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.

answer: the rate of diffusion increases with increase in temperature.

increase in temperature, increases the molecular/particles speed (kinetic energy. diffusion means movement of particles through the material.

generally, the heavier the particle the more it interacts with the environment and more the temperature matters. so higher temperature results in higher diffusion.