How Many Moles of Fe Ion Are in 5 mL of Fe(NO3)3 Solution?

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To determine the moles of Fe ion in a 5 mL solution of Fe(NO3)3 at a concentration of 0.200 mol/L, the calculation involves multiplying the concentration by the volume in liters. The correct calculation is 0.200 mol/L multiplied by 0.005 L, resulting in 0.001 moles of Fe ion. There is one Fe3+ ion for each formula unit of Fe(NO3)3, so no division is necessary. The final answer is 0.001 moles of Fe ion in the solution. Understanding the stoichiometry of the compound is crucial for accurate calculations.
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Homework Statement



If you have 5 mL of Fe(NO3)3(aq) at a concentration of 0.200 mol/L

How many moles of Fe ion do you have?

The Attempt at a Solution



Would it simply be (0.200) * (0.005) = answer


or would you have to divide that answer by three since one Fe per three NO3?

THANK YOU!
 
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There is only ONE Fe3+ ion for each Fe(NO3)3(aq). I think that answers your question.
 
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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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