Question

13.4 grams of iron (III) oxide reacts with 12.3 grams of carbon monoxide to produce 8.23 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.Please Help

Answer 1

1. write a reaction then balance it.

2. find the moles of iron produced by using the stoichiometric coefficients.

e.g. for a general reaction:

aA + bB \(\rightleftharpoons\) cC

where upper case are the species, and lower case are the coefficients,

\(\dfrac{n_A}{a}=\dfrac{n_B}{b}=\dfrac{n_C}{c}\)

from here, you can solve for moles then convert to grams.

The amount of grams you find here is the theoretical yield.

3. finding percent yield, use: \(\% yield=\dfrac{actual\;yield}{theoretical\;yield}*100\%\)

the units should both be the same, otherwise it won't work.

Answer 2

Fe2O3 + 3 CO-->2 Fe + 3 CO2

Answer 3

right?

Answer 4

yup, you now need to convert the masses given to moles and use their stoichiometric coefficients to build a ratio, like i stated above.

Answer 5

can u help with that please

Answer 6

convert to moles first

Answer 7

idk how

Answer 8

13.4 grams of iron (III) oxide reacts with 12.3 grams of carbon monoxide

\(n=\dfrac{m}{M}\)

where, n=moles, m=mass (in g), M=molar mass (in g/mol).

You'll find M on the periodic table

Answer 9

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Answer 10

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Answer 11

?

Answer 12

can you just do the question out so i can find the percent yield

Answer 13

i'm not going to do your work

Answer 14

I just need explanation, like a bit of a back and forth thing.

Answer 15

i wrote above how you can find the amount of moles of both reactants.

Answer 16

or can u add someone else to help me please?

Answer 17

ill give a medal

Answer 18

i'm trying to help you but you don't wanna do any work.

Answer 19

@Hero please help

Answer 20

@Chemistry please help