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Chemistry confusion ?
So idk how I would even begin to set up this question? Is it using limiting reactant ?
Fe+CuSO4------>FeSO4+Cu
If 0.5206 g of iron is reacted, how many moles of copper should be produced
2 Answers
- ChemTeamLv 78 years agoFavorite Answer
Since the problem is silent about the amount of CuSO4, we assume there is a sufficient amount of it. In essence, the iron is the limiting reagent.
Step 1: moles of iron:
0.5206 g / 55.845 g/mol = 0.00932223 mol
Step 2: use molar ratio:
The Fe to Cu molar ratio is 1 to 1.
1 is to 1 as 0.00932223 mol is to x
x = 0.00932223 mol of Cu
Since this is the desired answer, we round off to 4 sig figs:
0.009322 mol
Often, the problem will ask for the answer in grams.
Step 3: convert moles to grams:
0.00932223 mol times 63.546 g/mol = 0.5924 g (to four sig figs)
Source(s): ChemTeam - ?Lv 58 years ago
You would have to assume that Fe is the limiting reagent as nothing else has been stated.
Fe and Cu are in a 1:1 ratio so simply calculate the moles of Fe and this is the same as the number of moles of Cu produced.
Moles = Mass/RMM
There is the equation if you didn't know it.
