Consider the following chemical reaction: 3H2(g)+N2(g)→2NH3(g) How many grams of NH3 can be synthesized from 3.00 g of H2?

Answer 1

First check to see if the equation is balanced.

3H2+N2→2NH3

On the first side of the equation there are the following number of atoms of each substance:

H = 6

N = 2

One the second side of the equation there are the following number of atoms of each substance:

H = 6

N = 2

Since the number matches, this means the equation is balanced.

Next calculate the molar mass of each element to find the number of moles of H₂.

The atomic weight of H = 1.008 g/mol and N = 14.007 g/mol

This means the molar mass of H₂ is 2(1.008) = 2.016 g/mol

and NH₃ is 14.007 + 3(1.008) = 14.007 + 3. 024 = 17.031 g/mol

Then find the number of moles of H₂ in 3.00 g

3.00 g x 1 mole = 1.488 moles H₂

2.016 g

Use the ratio of H₂ to NH₃ (3 to 2) to find the number of moles of NH_3.

1.488 moles H₂ x 2 moles NH₃ = 0.992 moles NH₃

3 moles H₂

Now that the number of moles of NH₃ are known, the molar mass can be used to find the number of grams.

0.992 moles NH₃ x 17.031 g = 16.89 g NH₃

1 mole NH₃

16.89 g NH₃ is your final answer