Cell Target definition in science
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Answer: The percent yield of this combination reaction is 41.3 %
Explanation : Given,
Mass of = 5.0 g
Mass of = 10.0 g
Molar mass of = 23 g/mol
Molar mass of = 71 g/mol
First we have to calculate the moles of and
.
and,
Now we have to calculate the limiting and excess reagent.
The balanced chemical equation will be:
From the balanced reaction we conclude that
As, 2 mole of react with 1 mole of
So, 0.217 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of
From the reaction, we conclude that
As, 2 mole of react to give 2 mole of
So, 0.217 mole of react to give 0.217 mole of
Now we have to calculate the mass of
Molar mass of = 58.5 g/mole
Now we have to calculate the percent yield of this reaction.
Percent yield =
Actual yield = 5.24 g
Theoretical yield = 12.7 g
Percent yield =
Percent yield = 41.3 %
Therefore, the percent yield of this combination reaction is 41.3 %
Answer:
Left hand side:-
Carbon - 12
HYdrogen - 28
Oxygen - 38
Right hand side:-
Carbon - 12
Hydrogen - 28
Oxygen - 38
Since, the number of atoms each side are equal, the reaction is balanced.
Explanation:
The given reaction is:-
Left hand side:-
Carbon - 12
HYdrogen - 28
Oxygen - 38
Right hand side:-
Carbon - 12
Hydrogen - 28
Oxygen - 38
<u>Since, the number of atoms each side are equal, the reaction is balanced.</u>
Answer: D. 19.9 g hydrogen remains.
Explanation:
To calculate the moles, we use the equation:
a) moles of
b) moles of
According to stoichiometry :
1 mole of require 1 mole of
Thus 0.0787 moles of require=
of
Thus is the limiting reagent as it limits the formation of product and
acts as the excess reagent. (10.0-0.0787)= 9.92 moles of
are left unreacted.
Mass of
Thus 19.9 g of remains unreacted.