how many column of charge are required to produce 4.05g aluminium from Al2 from Al2O3
Answers
Answer:
Hope this will help you ❤
Explanation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
I'm not really sure I follow your calculations on this one.
For starters, a very quick way of figuring out which reactant will act as the limiting reagent when dealing with equal masses of the two reactants is to look at their molar masses.
When you're dealing with equal masses of two reactants, the reactant that has the greater molar mass will have the smallest number of moles present in the given mass.
In this case, iron (III) oxide has a molar mass of 159.7 g mol−1 and carbon monoxide has a molar mass of 28.01 g mol−1.
Right from the start, you should be able to tell that iron(III) oxide will be the limiting reagent because you have significantly more moles of carbon monoxide in 2.00 kg than moles of iron(III) oxide in 2.00 kg.
More specifically, you will have
2000g⋅1 mole Fe2O3159.7g=12.52 moles Fe2O3
2000g⋅1 mole CO28.01g=71.40 moles CO
If all the moles of iron(III) were to take part in the reaction, then the reaction would also consume
12.52moles Fe2