Question

For questions 2 to 4 d, consider two 2.00 L flasks, one of which contains 0.250 mole of O₂

gas at 50.0 deg C and the other of which contains 0.500 mole of H₂ gas at 50.0 deg C.  

a.    

In which flask is the ratio of molecular volume (volume occupied by the

                  molecules touching one another in a condensed state) to gaseous sample

                  volume (volume occupied by the entire gaseous sample) greater? (2 pt)

         b.    

What is the approximate value of these ratios? Explain. Calculation

                  not needed (4 pt)

         c.   

   In which sample do the molecules have higher average kinetic energy? Explain.

                  Calculation not needed (4 pt)

         d.   

   In which flask do the molecules have higher average speed? Explain.

                  Calculation not needed (4 pt)

Explain in detail please.

Answer 1

a. and b.

First flask contains O2 and second flask contains H2

Higheris the number of moles, higher is the ratio.

In first flask is the ratio of molecular volume (volume occupied by the molecules touching one another in a condensed state) to gaseous sample volume (volume occupied by the entire gaseous sample) greater.

The approximate value of these ratios is 2.

c.

Averae kinetic energy per molecule Since temperature is same, the average kinetic energy per molecule is same in both flasks.

d.

Average speed

At constant temperature

Second flask containing hydrogen has higher average speed as hydrogen has lower molar mass than oxygen.

d.