Cherylanne mixes together Chemical A and Chemical B in a test tube, forming Chemical C. The mixture instantly turns cool to the
2 answers:
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First we will calculate the number of moles of Iron:
, where n is the number of moles, m is the mass of iron in the reaction and M is the Atomic weight.
moles of Iron.
The same number of moles of Oxygen will take part in the reaction.
So
where 32 is the Atomical Weight of Oxygen (16 x 2).
=>
g
The same number of moles of Oxygen will take part in the reaction.
So
=>
The empirical formula of the compound : <u><em>RbO₂</em></u>
<h3>Further explanation</h3>Dulong and Petit's rule's rule, which says that the molar heat capacity, Cp, of a solid can be expressed as
Where N is the number of atoms per formula unit and R is the universal gas constant
While the value of R is:
R = 8.3144621 J / K · mol
then:
3R = 24.94 J / K · mol
Heat capactiy per gram of a compound containing rubidium and oxygen is 0.64 J · K⁻¹ · g⁻¹
We try the possible empirical formula from the composition of Rb and O
- Rb₂O
So the number of atoms: 3 (Rb = 2 atoms, O = 1 atom)
Then the value of the Cp:
Molar mass Rb₂O = 2.85.5 + 1.16 = 187 g/mol
Then this empirical formula Rb₂O is not appropriate
- RbO₂
So the number of atoms: 3 (Rb = 1 atom, O = 2 atoms)
Then the value of the Cp:
Molar mass RbO₂ = 1.85.5 + 2.16 = 117.5 g / mol
Then this empirical formula RbO₂ is appropriate
<h3>Learn more </h3>
chemical bond
ionic bonding
electron dots
Keywords: an empirical formula,compound, gas constant, Dulong and Petit's rule,the molar heat capacity
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