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