Assuming the temperature and volume remain constant, changes to the pressure in

Question

Assuming the temperature and volume remain constant, changes to the pressure in the reaction vessel will directly correspond to changes in the number of moles based on the ideal gas law.

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 298 K and 2.00 L, respectively. If the pressure was 8.02 atm prior to the reaction, what would be the expected pressure after the reaction was completed?

Explanation / Answer

The reaction is given as :

N2 + 3H2 = 2NH3

So the reaction had 4 moles of gaseous reactants in the start of reaction that accounted for 8.02 atm

Now the number of moles in products is 2 , so the pressure will be given as :
p1 n2 = p2 n1

where p is pressure and n is number of moles.

So putting all the value we get :

8.02 x 2 = p2 x 4

p2 = 4.01 atm

So the expected pressure after the completion of reaction is 4.01 atm

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