Consider the combustion of CH4.
Suppose 2.8 mole of CH4 are allowed to react with 5.0 mole of O2.
How many grams of CO2 can be made from this reaction?
CH4 + 2O2 ==> CO2 + 2H2O
Answers
Explanation:
There are different methods of finding the limiting reactant, here is the simplest to my opinion.
The reaction is:
C
H
4
(
g
)
+
2
O
2
(
g
)
→
C
O
2
(
g
)
+
2
H
2
O
(
g
)
Find the molar ratio between the experimental number of moles and theoretical number of moles of the reactants:
For
C
H
4
:
2.8
m
o
l
1
m
o
l
=
2.8
.
The
1
mol
is taking from the coefficient of
C
H
4
from the balanced equation.
For
O
2
:
3
m
o
l
2
m
o
l
=
1.5
.
The
2
mol
is taking from the coefficient of
O
2
from the balanced equation.
The reactant that gives the smaller molar ratio is the limiting reactant which is in this case the oxygen
O
2
More Explanation:
To consume the
2.8
moles of
C
H
4
we need
5.6
moles of
O
2
since the molar ratio is 1:2. We have only
3
moles of
O
2
; therefore,
O
2
is the limiting reactant.
I hope you will understand my answer so make me as brainliest please