Question

In an experiment 1.0912 g of ferric oxide is reacted with 0.4373 g of carbon monoxide gas according to the equation:
Fe2O3 + CO ==> Fe + CO2.

A. What is the limiting reactant?
B. What mass of the other reactant is in exess?
C. What mass of iron is produced?

Answer 1

Well first you need to balance the equation.

Answer 2

please can you help me balance the equation

Answer 3

look at number of each atom on left side and on right side
try to make it so number of atoms on right side is equal to left side

Answer 4

help me this is my first time of doing chemtry

Answer 5

well look
Fe2O3 + CO ==> Fe + CO2.

lets take O
look at left of the arrow
tell me how many O atoms do u see?

Answer 6

u wrote same thing that was there
balance ittt

Answer 7

i see two o

Answer 8

why? i said LEFT
where on left side u see 2?

Answer 9

why are you jumping <.<
where is the other part of the reaction?

Answer 10

you did it on your own?

Answer 11

well done :) yes that is right :)

Answer 12

find mole of Fe2O3 and mole of CO
their masses are given

Answer 13

mole= mass/ molecular mass

Answer 14

is this correct 1/ 291.7167 g/mol

Answer 15

why 1 divided by that?
i suggest you to write the whole mass that they gave, i mean with all decimals

Answer 16

is that the right answer 291.7167 g/mol

Answer 17

i don't have periodic table near me
u do know how to take molecular mass right?
if so then yeah you are right probably

Answer 18

sorry gtg @sweetburger will help out with the rest :)

Answer 19

ok thank u so much for helping this is my first time of being here how do i tell sweetburger to help me

Answer 20

are u with me

Answer 21

i'll just quickly tell the whole work
A- find moles of both reactants => Compound with smallest mole is Limiting reagent
B- here you just do some math comparison stuff
C- you take the mole of the limiting reagent and check the ratio between limiting reagent and Fe (meaning look at coefficients) and the use this ratio to find mole of Fe
from mole using formula mass=mole* Molecular mass get the mass of Fe

@sweetburger will explain these steps in depth
good luck ❤

Answer 22

thank you so much may god bless you

Answer 23

hehe no probs :)))

Answer 24

and thank you ❤

Answer 25

bye have a wounderfull day

Answer 26

night rather lol :))

Answer 27

someone help

Answer 28

Did you balance this yet?

Answer 29

Step 1: Balance Your Chemical Equation
Write down the number of atoms that you have on each side of the equation.
Look at the subscripts next to each atom to find the number of atoms in the equation.
Fe:2 Fe:1
O:4 O:2
C:1 C:1
Start with Oxygen, Carbon and Iron. Carbon Monoxide is a reducing, it would take out all the oxygen atoms from iron.
*2 to the Oxygen in CO2 of the product side
Fe2O3(s) + CO(g) --> Fe(s) + 2CO2(g)
*2 to CO on the reactant side to balance
Fe2O3(s) + 2CO(g) --> Fe(s) + 2CO2
Change the Oxygen by *3 instead of 2
Fe2O3(s) + 2CO(g) --> Fe(s) + 3CO2
Change the Oxygen and Carbon on the reactant side
Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2
Balance Iron on both side by *2 on reactant side and product side.
Fe2O3(s) + 3CO(g) --> 2Fe(s) + 3CO2(g)

Number of Moles=Mass(g)/Molar Mass(g/mol)
Molar Mass:(55.8*2)+(16*3)=159.6
1.0912/159.6=0.00687 moles of Fe2O3
Molar Mass: 0.4373/(12+16)=0.0156 moles of CO
Look at the Mole Ratio of Fe2O3 to CO based on CO mass
1:3
0.00687:x
x=0.02061 mole of CO, but there is 0.0156
Look At the Mole Ratio of Fe2O3 to CO based on Fe2O3
1:3
x:0.0156
x=0.00299
This is less thats whats required to react and therefore CO is the limiting reagent.
The excess reactant is FeO3
0.00687-0.00299=0.00388 Moles are in Excess
0.00388*159.6=Mass
Mass:0.61692 grams of iron
Lets get to the last part of your question
Look At the Mole Ratio of CO:Fe
3:2
0.0156:x
X:0.0156*2/3=0.0104 Moles of iron Are produced.
Number of moles=Mass(g)/Molar Mass(g/mol)
0.0104*55.8=Mass(g)

Answer 30

The excess reactant is Fe2O3*
Well done @Abmon98 :DDD

Answer 31

Thank you @Somy and sorry for that :/

Answer 32

please which one is the right answer

Answer 33

:)))