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2 years ago

A 1.000-g sample of lead shot reacted with oxygen to give 1.077 g of product. Calculate the empirical formula of the lead oxide

Chemistry

2 answers:

Alex_Xolod [135]2 years ago

7 0

The empirical formula of lead oxide is PbO

<u><em>Calculation</em></u>

Step 1: find the mass of oxygen that reacted

=mass of the product- mass of lead

= 1.077 g - 1.000 =0.077 g

Step 2: find the mole of each reactant

moles = mass/molar mass

the molar mass of Pb =207 g/mol while that of O = 16g/mol from periodic table

moles of lead(Pb) is therefore = 1.000 g / 207 g/mol =0.0048 moles

moles of O2 =0.077g/16 g/mol =0.0048 moles

Step 3: find the mole ratio

that is divide each mole by smallest number of mole (0.0048)

Pb = 0.0048/0.0048 =1

O=0.0048/0.0048 =1

from mole ratio above in 1 atom of Pb of the product we have 1 atom of O therefore the empirical formula is PbO

Evgesh-ka [11]2 years ago

3 0

It mean it consisted of 1 g of lead and 0.077 g of O2.
divide these numbers by molar mas.
1/82=0.012 Pb /0.004 = 3
0.077/16= 0.004 O /0.004 =1
Pb3O

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