Answer:
The empirical formula is = 
The molecular formula = 
Explanation:
% of C = 10.13
Molar mass of C = 12.0107 g/mol
% moles of C = 10.13 / 12.0107 = 0.8434
% of Cl = 89.87
Molar mass of Cl = 35.453 g/mol
% moles of Cl = 89.87 / 35.453 = 2.5349
Taking the simplest ratio for C and Cl as:
0.8434 : 2.5349
= 1 : 3
The empirical formula is =
Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.
Thus,
Molecular mass = n × Empirical mass
Where, n is any positive number from 1, 2, 3...
Mass from the Empirical formula = 12*1 + 3*35.5 = 118.5 g/mol
Molar mass = 237 g/mol
So,
Molecular mass = n × Empirical mass
237 = n × 118.5
⇒ n ≅ 2
The molecular formula =
How it looks. basically the thing that tells you how it change. for example if an ice cube was melted (heat), it only changed physically not chemically as the h20 molecules are still there. however lets say you burn woos— you cant get that would back. its ash now and it has changed chemically.
Dilution<span> is when you decrease the concentration of a </span>solution<span> by adding a solvent. As a result, if you want to </span>dilute<span> salt water, just add water. ... Add more solute until it quits dissolving. That point at which a solute quits dissolving is the point at which it's </span>saturated<span>.</span>
Answer:
D. 91.98K
Explanation:
The General Gas Law equation is given by,
From the question,
the initial pressure,
the initial volume,
the final temperature,
the final pressure,
the final volume,
Making
the subject of the expression, we obtain
By substitution,
Hence the initial temperature was 91.98 K
of octane had been converted to carbon dioxide CO₂.
<h3>Explanation</h3>
Octane has a molar mass of
1.000 gallon of this fuel would have a mass of 2.650 kilograms or 
, which corresponds to 
of octane.
Octane undergoes complete combustion to produce carbon dioxide and water by the following equation:
An incomplete combustion of octane that gives rise to carbon monoxide and water but no carbon dioxide would consume not as much oxygen:
The mass of the product mixture is 
heavier than that of the octane supplied. Thus 
of oxygen were consumed in the combustion. There are 
of oxygen molecules in 
of oxygen.
Let the number of moles of octane that had undergone complete combustion as seen in the first equation be 
(
). The number of moles of octane that had undergone incomplete combustion through the second equation would thus equal 
.
25 moles of oxygen gas is consumed for every two moles of octane that had undergone complete combustion and 17 moles if the combustion is incomplete.
Therefore 
out of the 23.2 moles of octane had undergone complete combustion to produce carbon dioxide.
