The fertilizer ammonium sulfate is prepared commercially by the reaction of ammonia with sulfuric acid.
Calculate the mass of (NH4)2SO4 that would be formed from 34.0 g NH3.
Calculate the mass of (NH4)2SO4 that would be formed from 34.0 g NH3.
| reaction | 2NH3(g) | + | H2SO4(l) |  | (NH4)l2SO4(s) |
| known | unknown | ||||
| masses given /g | 34.0 | ||||
divide by molar mass:  |  M(NH3) = 17.0 g mol–1 | ||||
| amount of known/mol | 2.00 | ||||
| divide by the coefficient on given substance in the balanced equation |  | Warning! Do not round early! Correct answers have 3 sig figs as in data. | |||
| predicted amount of reaction/mol | 1.00 | ||||
| multiply by the coefficient on unknown substance in the balanced equation |  | ||||
| predicted amount of unknown/mol | 1.00 | ||||
| multiply by molar mass: m = n × M | M((NH4)2SO4) 132 g mol–1 | | |||
| predicted mass of unknown/g | 132 | ||||