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

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 [tex]1.00x10^{3} Kg[/tex] of carbon has [tex]8.33x10^{4} mol[/tex] of C

Remember: mol(n)

[tex]n=\frac{sample mass}{molar mass}[/tex]

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 [tex]8.33x10^{4} mol[/tex] of CO(NH3)2

[tex]8.33x10^{4} mol[/tex] of CO(NH3)2 has [tex]5.00x10^{3} Kg[/tex]

[tex]Sample mass = n*molar mass[/tex]

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

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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