Question about unknown type of metal ion

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To determine the minimum volume of Cu2+ solution needed to completely react with 1.0 g of iron, it is essential to consider the stoichiometry of the reactions involving both Fe2+ and Fe3+. The first reaction shows that one mole of iron reacts with one mole of Cu2+, while the second reaction indicates that two moles of iron react with three moles of Cu2+. The molar concentration of the CuSO4 solution is given as 1.0 M, which is necessary for calculating the required moles of Cu2+. The calculation should focus on the reaction that utilizes the least amount of iron, which will dictate the volume of Cu2+ solution needed for complete reaction. Understanding these relationships will clarify the approach to solving the problem.
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Homework Statement


we are mixing CuSo4 (Cu2+) with an iron (Fe) powder and we are trying to determine whether Fe2+ forms or Fe3+
now the question is :
suppose that 1.0 g of iron is used in the experiment. what is the minimum volume of Cu2+ solution that must be added in order to completely react the iron? should this calculation be based on the reaction of Fe2+ or Fe3+ with Cu2+?

Homework Equations


Fe(s) + Cu2+(aq) ---> Fe2+(aq) + Cu(s)
2Fe(s) + 3Cu2+ ---> 2Fe3+(aq) + 3Cu(s)

The Attempt at a Solution


are we supposed to determine which equation uses the least Fe? and if so how are we supposed to change that mass or moles of Cu2+(aq) into volume?
id really appreciate some help :)
 
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You need molar concentration of copper sulfate to calculate moles.
 
oops sorry to include that its a 1.0M solution cuso4
 
Show how you are approaching the question, it is relatively easy and I have no idea where and why do you get lost.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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