Question

How many grams of H2 are necessary to react completely with 50g of N2?

Answer 1

The address the reduction equation...`1/2N_2(g) + 3/2H_2(g)rarrNH_3(g)`

Explanation:

Now we COULD be making hydrazine `H_2N-NH_2`....but given the context, they want to consider complete reduction to ammonia (anyway this is something to point out to your instructor)... And so we require THREE EQUIV of dihydrogen gas...

`n_(N_2)=(50.0*g)/(28.02*g*mol^-1)=1.78*mol`

And `n_(H_2)=(50.0*g)/(28.02*g*mol^-1)xx3=5.35*mol`

This represents a mass of `5.35*molxx2.02*g*mol^-1=10.7*g`.

And if `p_(N_2)=1*atm`, what pressure of dihydrogen does this represent?