Basis of the calculation: 100g
For Carbon:
Mass of carbon = (100 g)(0.80) = 80 g
Number of moles of carbon = (80 g)(1 mole / 12g) = 20/3
For Hydrogen:
Mass of hydrogen = (100 g)(0.20) = 20 g
Number of moles of hydrogen = (20 g)(1 mole / 1 g) = 20
Translating the answer to the formula of the substance,
C20/3H20
Dividing the answer,
CH3
The molar mass of the empirical formula is:
12 + 3 = 15 g/mol
Since, the molar mass given for the molecular formula is 30.069 g/mol, the molecular equation is,
C2H6
ANSWER: C2H6
Answer:1. 
2. 
3.
4. 
5. 
Explanation:
Molecular formula is the chemical formula which depicts the actual number of atoms of each element present in the compound.
Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.
1. 
has empirical formula of
2. 
has empirical formula of
3. has empirical formula of
4. has empirical formula of
5. 
has empirical formula of
Speed = Wavelength x Frequency
and frequency = 1/Period
Speed = Wavelength/Period
Speed = .5 * 2
Speed = 1 m/s
The balanced chemical reaction is written as:
<span>2Al2O3 = 4Al + 3O2
We are given the amount of aluminum oxide used in the reaction. This will be the starting point for the calculations. We do as follows:
26.5 mol Al2O3 ( 3 mol O2 / 2 mol Al2O3 ) = 39.75 mol O2 produced</span>
