Suppose the reaction between nitrogen and hydrogen was run according to the amounts presented in part a, and the temperature and volume were constant at values of 303 k and 2.00 l, respectively. if the pressure was 10.4 atm prior to the reaction, what would be the expected pressure after the reaction was completed?

Explanation:

Assuming that moles of nitrogen present are 0.227 and moles of hydrogen are 0.681. And, initially there are 0.908 moles of gas particles.

This means that, for

 moles of + moles of = 0.908 mol

Since, 2 moles of = = 0.454 mol

As it is known that the ideal gas equation  is PV = nRT

And, as the temperature and volume were kept constant, so we can write

        =

          =

        =

                            = 5.2 atm

Therefore, we can conclude that the expected pressure after the reaction was completed is 5.2 atm.

20 drops hope this