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 -> NH3

Answer 1

Answer:- No, the company would not be able to full fill the order.

Solution:- The balanced equation for the formation of ammonia by the reaction of hydrogen with nitrogen is:

`3H_2+N_2\rightarrow 2NH_3`

We have been given with 22000 grams of nitrogen and 1000 grams of hydrogen. Let's convert grams of each to moles:

moles of nitrogen =
`22000g N_2((1mol)/(28g))`

moles of nitrogen = 785.71 mol

moles of hydrogen =
`1000g H_2((1mol)/(2g))`

moles of hydrogen = 500 mol

From balanced equation 3 moles of hydrogen react with 1 mol of nitrogen. Let's calculate how many moles of nitrogen would react with 500 mol of hydrogen:

`500mol H_2((1mol N_2)/(3mol H_2))`

=
`166.67 mol N_2`

166.67 moles of nitrogen are required and 785.71 moles of it are available. It means nitrogen is in excess and hydrogen is limiting. Product yield depends on limiting reactant. So, let's calculate the amount of ammonia formed from moles of hydrogen as:

`500mol H_2((2mol NH_3)/(3mol H_2))((17g NH_3)/(1mol NH_3))`

= 5666.67g of ammonia

let's convert the grams of ammonia to number of batches as:

`5666.67g NH_3((1 batch)/(175g NH_3))`

= 32 batches

Company needs to make 70 batches of ammonia but from given amounts of hydrogen and nitrogen only 32 batches could be made. It means the company would not be able to full fill the order.