Question

A chemical company makes ammonia by reacting nitrogen with hydrogen. The company needs to make 70 batches of ammonia for a client. Each batch contains 175 grams. They have 22,000 grams of N2 and 1000 grams of H2. Will they be able to make enough ammonia to fill the order? (You may have to balance the equation.)H2 + N2 -> NH3A. No, the ammonia will run out first.B. No, the hydrogen will run out first.C. Yes, and there will be extra unreacted hydrogen left over.D. Yes, and there will be extra unreacted nitrogen left over.

Answer 1

Step-by-step explanation:

First, we need to write the equation balanced:

N2 + 3 H2 --> 2 NH3

If 1 batch contains 175 grams:

1 batch --- 175 grams

70 batches ---- x

x = 12,250 g of ammonia needs to be produced.

Now let's transform 22,000 g of N2 and 1,000 grams of H2 into moles. For this, we use the following formula:

n = m/MM

MM of N2: 28 g/mol

n = 22,000/28

n = 785.7 moles

MM of H2: 2 g/mol

n = 1000/2

n = 500 moles

So it means that H2 is the limiting reactant, because the stoichometry of N2 and H2 is 1:3.

So:

3 moles of H2 --- 2 moles of NH3

500 moles of H2 --- x moles of NH3

x = 333.33 moles of NH3

Now we transform this value into grams:

m = n*MM

MM of NH3 = 17 g/mol

m = 333.33*17

m = 5,666.6 g

With 22,000 g of N2 and 1000 g of H2 it will be produced 5,666.6 g of NH3.

We need to produce 12,250 g of ammonia.

So:

Answer: B. No, the hydrogen will run out first.