2C3H6 + 2NH3 + 3O2 -> 2C3H3N + 6H2O?
What mass of acrylonitrile can be produced from a mixture of 1.15kg of propylene, 1.72kg of ammonia, and 1.99kg of oxygen?
What mass of water is produced?
What mass of propylene is left over?
What mass of ammonia is left over?
What mass of oxygen is left over?
Please help i dont know what to do.
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Convert between mass and moles. For example, there is 1.99kg of O2 in the beginning. Convert that to moles (use the molar mass on the periodic table, I believe O2 is 32 grams per mole), convert that to the amount of water prodced (there are twice as many moles of water than oxygen) and convert this new mole value to mass using the molar mass of water (18 grams per mole I think).
Repeat for other values.
Under the balanced equation write:
2 moles + 2 moles + 3 moles -> 2 moles + 6 moles
Then work out how many moles propylene, ammonia and O2 are in the masses given. This will let you see which reactant is the limiting factor - once that's all used up, reaction stops (eg if you have five moles propylene, four moles ammonia, and seven moles O2, all ammonia would reac but only four moles propylene and six moles O2 could react).
Hope that's enough to get you started.
At least one of your answers will be "none"