Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N 2 (g) 3H 2 (g) 2NH3 (g) If the reaction yield is 87.5%, how many moles of N 2 are needed to produce 3.00 mol of NH 3

We need 1.714 moles N2

Explanation:

Step 1: Data given

The reaction yield = 87.5 %

Number of moles NH3 produced = 3.00 moles

Step 2: The balanced equation

N2 (g) + 3H2 (g) →2NH3 (g)

Step 3: Calculate moles N2

For 2 moles NH3 produced we need 1 mol N2 and 3 moles H2

This means, if the yield was 100%, for 3.00 moles NH3 produced, we need 1.5 moles N2

For a 87.5 % yield:

we need more N2, increased by a ratio of 100/87.5.

100/87.5 * 1.5 = 1.714 moles N2