Question

When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide.

C(s)+O₂(g) -> CO₂(g)

However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result.

2C(s)+O₂(g) -> 2CO(g)

What mass of each product is expected when a 8.60 g sample of pure carbon is burned under each of these conditions?

____g CO2

____ g CO

Answer 1

Balanced chemical equation,

C(s)              +          O₂(g)             ---->           CO₂(g)

12.0 g/mol              32.0 g/mol                      44.0 g/mol

=> 12.0 g C form    -------->     44.0 g CO2

        8.60 g C form --------->   x g CO2 (cross multiplication of these two gives)

x = (8.60*44.0) / 12.0

x = 31.5 g CO2 is formed

A:- The mass of CO2 formed from 8.60 g sample of pure carbon is burned = 31.5 g CO2

2C(s)          +              O₂(g) ---->                2CO(g)

2*12.0 g/mol                 32.0 g/mol                            2*28.0 g/mol

=> 2*12.0 g C form    ------->   2*28.0 g CO

      8.60 g C form      --------->   x g CO (cross multiplication of these two gives)

x = (8.60*2*28.0) / (2*12.0)

x = 20.1 g CO formed

A:- The mass of CO formed from 8.60 g sample of pure carbon is burned = 20.1 g CO