Question

Urea is manufactured on larg 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 the combustion of 1.00 x 103 kg of carbon followed by the reaction?

CO2 + 2NH3 ? CO(NH2)2 + H2O

Answer 1

`5.00x10^(3)  Kg`

Step-by-step explanation:

There are two reactions taking place and the product of the first is a reactant at the other, so writing down the balanced chemical equations is the first step in determinimg the proportions

1) C + O2 → CO2

1. Molar mass C = 12.0107 g/mol

2. Number of moles
`1.00x10^(3)  Kg` of carbon has
`8.33x10^(4)  mol` of C

Remember: mol(n)

`n=(sample mass)/(molar mass)`

2) CO2 + 2NH3 → CO(NH3)2 + H2O

1. Molar mass CO(NH3)2 = 60.02 g/mol

2. Proportions the urea syntheres has a proportion of 1:1 with carbon dioxyde, so there is
`8.33x10^(4)  mol` of CO(NH3)2

`8.33x10^(4)  mol` of CO(NH3)2 has
`5.00x10^(3)  Kg`

`Sample mass = n*molar mass`