anonymous
  • anonymous
I need help on two questions on my chemistry homework
Chemistry
  • Stacey Warren - Expert brainly.com
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jamiebookeater
  • jamiebookeater
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anonymous
  • anonymous
If 12.6 grams of iron (III) oxide reacts with 9.65 grams of carbon monoxide to produce 7.23 g of pure iron, what are the theoretical yield and percent yield of this reaction? Be sure to show the work that you did to solve this problem. unbalanced equation: Fe2O3 + CO yields Fe + CO2
anonymous
  • anonymous
and I have another question
anonymous
  • anonymous
If 143 grams of chromium react with an excess of oxygen, as shown in the balanced chemical equation below, how many grams of chromium oxide can be formed? Please show all your work for the calculations for full credit. 4Cr + 3O2 yields 2Cr2O3

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aaronq
  • aaronq
All stoichiometry problems are essentially the same. This is how to find the theoretical yield. General Scheme: \(\sf \large 1.\)First write and balance an equation for the process described. \(\sf \large 2.\)Next, use the stoichiometric coefficients to find moles produced. \(\sf \large 3.\) Set up a ratio using the species of interest, like so: e.g. for a general reaction: \(\sf \large \color{red}{a}A + \color{blue}{b}B \rightleftharpoons \color{green}{c}C\) where upper case are the species (A,B,C), and lower case (a,b,c) are the coefficients , \(\sf \dfrac{n_A}{\color{red}{a}}=\dfrac{n_B}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\) 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: \(\sf\dfrac{2}{\color{blue}{b}}=\dfrac{n_C}{\color{green}{c}}\rightarrow n_C=\dfrac{2*\color{green}{c}}{\color{blue}{b}}\) \(\sf \large 4.\) Solve ---- Then, Percent yield =\( \sf \dfrac{|theoretical-actual ~yield| }{theoretical }*100 \% \) The "actual yield" is given in the question.
anonymous
  • anonymous
Can u help me solve them
aaronq
  • aaronq
I can tell you if you're doing it right or not, but you have to post your work in order for me to do that.
anonymous
  • anonymous
Im really confused and have turn in my homework soon
anonymous
  • anonymous
4 Cr + 3 O2 → 2 Cr2O3 (143 g Cr) / (51.99616 g Cr/mol) x (2 mol Cr2O3 / 4 mol Cr) x (151.99061 g Cr2O3/mol) = 209 g Cr2O3
aaronq
  • aaronq
so you wanna do the second one? thats right (assuming you didn't make a mistake with the arithmetic)
anonymous
  • anonymous
for the second one im really confused
aaronq
  • aaronq
btw, i know you're copying and pasting, copied that from here https://ca.answers.yahoo.com/question/index?qid=20130420150711AAXIf8o
aaronq
  • aaronq
you're not gonnna learn anything by doing that..
anonymous
  • anonymous
can u help me then
aaronq
  • aaronq
Is what i gave you initially (the scheme) not sufficient? What else do you need?
anonymous
  • anonymous
can u help me with at least the first onelike do i together
aaronq
  • aaronq
Okay you start
anonymous
  • anonymous
unbalanced is Fe2O3 + CO yields Fe + CO2
aaronq
  • aaronq
k now balance it
anonymous
  • anonymous
Fe2O3 + 3 CO = 2 Fe + 3 CO2
aaronq
  • aaronq
Awesome. Now we need to find the moles of each (and determine the limiting reactant - the one with least moles). The formula is \(\sf moles=\dfrac{mass}{Molar~mass}\) lets do iron(III) oxide first, the mass is 12.6 grams and the molar mass is 159.69 g/mol
anonymous
  • anonymous
ok
aaronq
  • aaronq
what did you get?

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