For the following reaction, calculate how many moles of each product are formed when 0.356 moles of pbs completely react. assume there is an excess of oxygen.
2pbss+3o2g→2pbos+2so2g

0.356 moles of each products (PbO and SO2) are formed.

Explanation:

First step is to write out the equation and ensure it is balanced before proceeding.

2PbSs + 3O2g → 2PbOs + 2SO2g

2            3            2              2

The equation above is balanced because there are equal number of atoms of elemenents on both sides of the arrow.

By stating that oxygen is in excess, this tells that PbS is the limiting reactant (i.e the amount of products formed depends on it) and not on oxygen.

From the equation;

The products formed are PbO and SO2.

For PbO, it requires 2 moles of PbS to react completely in order to form 2 moles of PbO.

For SO2, it requres 2 moles of PbS to react completely in order to form 2 moles of SO2.

This is gotten from the equation.

PbO

2 moles = 2 moles

0.356 moles = x

upon cross multiplication, we are left with;

x = (0.356 * 2) / 2 = 0.356 moles

SO2

2 moles = 2 moles

0.356 moles = x

upon cross multiplication, we are left with;

x = (0.356 * 2) / 2 = 0.356 moles

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