Question

Question #3: What mass of FeC2O4 should be obtained?
*attached I have the questions, along with my work up until question 3.

Answer 1

okay, so for #2, you \(\color{red}{don't}\) need to add the moles found in #1.

For #3, when you find the limiting reagent, you divide the moles of a given reactant by it's stoichiometric coefficient in the balanced equation. Whichever is less is the limiting reactant.

Answer 2

i just noticed both of the coefficient are 1, so the limiting reactant is the one with less moles (i.e. Fe...)

Answer 3

@aaronq your my lifesaver! Chemistry is not my favorite subject :/ yay so I was able to get the limiting reagent correctly! but i just noticed noticed i wrote question #3, when really my question was about #4!

Answer 4

ohh okay, sweet. Okay, so use the moles of the limiting reagent.
Use the stoichiometric coefficients to find moles produced.
Set up a ratio using the species of interest, like so:

e.g. for a general reaction:

\(\color{red}{a}A + \color{blue}{b}B\) \(\rightleftharpoons\) \( \color{green}{c}C\)

where upper case are the species (A,B,C), and lower case (a,b,c) are the coefficients ,

\(\dfrac{n_A}{\color{red}{a}}=\dfrac{n_B}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\)

From here you can isolate what you need.
For example: if you have 2 moles of B, how many moles of C can you produce?

solve algebraically: \(\dfrac{2}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\rightarrow n_C=\dfrac{2*\color{green}{c}}{\color{blue}{b}}\)

Answer 5

then convert to mass (which i'm sure you know how to do).

Answer 6

well ok, would this mean the answer in moles would be the same as the limiting reagent 5.2e-3?

Answer 7

indeed.

Answer 8

:o yes! and from there i just multiply by the molar mass of FeC2O4

Answer 9

yep!

Answer 10

:D yay. thank you so much for your help!

Answer 11

no problem! anytime