Question

Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO2 produced by combustion of 1.00 × 10^3 kg of carbon followed by the reaction? CO2 (g) + 2NH3 (g) ⟶ CO (NH2 )2 (s) + H2 O(l)

Answer 1

The mass of urea that can be manufactured is 5,000,832.65g.

Step-by-step explanation:

1st) It is necessary to balance the chemical reaction:

`CO_2+2NH_3\rightarrow CO(NH_2)_2+H_2O`

From the balanced reaction we know that from 1 mole of CO2, we obtain 1 mole of urea.

2nd) We have to calculate the amount of CO2 that we have, if there are 1.00x10^3 kg (1,000,000 g) of carbon:

- CO2 molar mass: 44.01g/mol

- C atomic mass: 12.01g/mol

In 44.01g of CO2, there are 12.01g of carbon (C). With a mathematical rule of three we can calculate the amount of CO2:

`\begin{gathered} 12.01gC-44.01gCO_2 \\ 1,000,000gC-x=(1,000,000gC*44.01gCO_2)/(12.01gC) \\ x=3,664,446.3gCO_2 \end{gathered}`

There are 3,664,446.3g of CO2 from 1,000,000g of C.

3rd) From the stoichiometry of the reaction, we know that from 44.01g (1 mole) of CO2, we can obtain 1 mole of urea (urea molar mass: 60.06g/mol). With a mathematical rule of three we can calculate the mass of urea that can be manufactured from 3,664,446.3g of CO2:

`\begin{gathered} 44.01gCO_2-60.06gUrea \\ 3,664,446.3gCO_2-x=(3,664,446.3gCO_2*60.06gUrea)/(44.01gCO_2) \\ x=5,000,832.65gUrea \end{gathered}`

So, the mass of urea that can be manufactured is 5,000,832.65g.