Question

Urea, NH₂CONH₂, is manufactured from ammonia and carbon dioxide according to the following equation:
`2 NH_3 (g) + CO_2 (g) \rightarrow NH_2CONH_2(aq) + H_2O (l)`What volume of ammonia gas at 25 °C and 1.5 atm is needed to make 500g of urea?

Answer 1

271.2 liters are needed to make 500g of urea

Step-by-step explanation:

2NH3 (g) + CO2 (g) → H2O (l) + NH2CONH2 (aq)

Molar mass of Urea: 60.06 g/m

Mass / molar mass : Moles

500 g / 60.06 g/m : 8.32 moles

Finally we have to make 8.32 moles of urea.

We start with the reaction, where 2 moles of ammonia reacts with 1 mol of carbon dioxide to make 1 mol of urea and water so:

-As 1 mol of urea comes from 2 moles of ammonia

How many moles of ammonia, do we need to make 8.32 moles of urea.

1 mol of urea ____ 2 moles NH3

8.32 moles of urea ___ 16.6 moles of NH3

We need the double, by the chemical equation.

Now that we know our needed moles, we can know the volume by the Ideal Gas law equation.

P.V = n.R.T

1.5 atm . V = 16.6 moles . 0.082 L.atm/K.mol . 298K

V = ( 16.6 moles . 0.082 L.atm/K.mol . 298K) / 1.5 atm

V = 271,2 L.