14.8k views
0 votes
What mass (in g) of nitrogen are needed to react completely with 5.8 g of hydrogen?

What mass (in g) of nitrogen are needed to react completely with 5.8 g of hydrogen-example-1
User Krul
by
7.1k points

1 Answer

4 votes

Answer:

We have the following chemical reaction:


N_2+3H_2\rightarrow2NH_3

First we calculate the moles of hydrogen that react. For this we use its molar mass:


M_(H_2)=2.1(g)/(mol)=2(g)/(mol)
n_(H_2)=(5.8g)/(2(g)/(mol))=2.9mol

Now, we know that for every 3 moles of H2 we need 1 mol of N2, so we calculate the moles of N2:


n_(N_2)=2.9mol_(H2)(1mol_(N2))/(3mol_(H2))=0.97mol

And now we use the nitrogen's molar mass to calculate the grams:


M_(N_2)=2.14(g)/(mol)=28(g)/(mol)
m_(N2)=0.97mol.28(g)/(mol)=27g

So the answer is 27g

User LachlanO
by
6.1k points