What is true regarding the calculation in redox titration? group of answer choices moles of the oxidant equal mole of the reduct
1 answer:
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Answer:
0.55 atm
Explanation:
First of all, we need to calculate the number of moles corresponding to 1.00 g of carbon dioxide. This is given by
where
m = 1.00 g is the mass of the gas
Mm = 44.0 g/mol is the molar mass of the gas
Substituting,
Now we can find the pressure of the gas by using the ideal gas law:
where
p is the gas pressure
V = 1.00 L is the volume
n = 0.0227 mol is the number of moles
R = 0.082 L/(atm K mol) is the gas constant
T = 25.0 C + 273 = 298 K is the temperature of the gas
Solving the formula for p, we find
What is Chemical Reaction?
A chemical reaction is the chemical transformation of one set of chemical components into another.
Main Content
Mass of aluminium sulfide is 158g
Mass of water is 131g
The chemical reaction:
First, balance the chemical equation
Aluminium sulfide has a molar mass of 150.16 g/mol and water has a molar mass of 18.02 g/mol. As a result, the moles of aluminum sulfide are computed as follows:
From the chemical reaction , the ratio of molar is 3mol So, the moles of hydrogen sulfide are:
= 7.26mol
From the chemical reaction, the molar ratio is 3 mol mol
So, the moles of hydrogen sulfide are:
Moles of formed = 7.26 mol
Th liming reactant is beacuse the mass of
forms less product than water. Therefore, the maximum number of moles of
is 3.15 mol. We know that molar mass of
is 34.10g/mol. So, the maximum mass of
formed is,
Molar mass of
= 3.15 mol 34.10g/mol
= 107.4g
Now, multiplying the number of moles of by the molar ratio between
and
which is 6mol
we get the number of moles of
reacted.
Moles of reacted = 1.05 mol
= 6.31 mol
The mass of is,
= 6.31 mol
18.02g/ mol
= 114g
On subtracting, the mass of reacted from the given mass of
is,
= (131-114)g
= 17g
Hence, the excess remaining reactant is 17g
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