When 3.0 g of carbon is burnt in 8.00 g oxygen, 11.00 g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00 g of carbon is burnt in 50.00 g of oxygen? Which law of chemical combination will govern your answer?

Explanation

Carbon and oxygen react to form carbon dioxide accordin to the equation
`"Carbon(C)"+"Oxygen"(O_(2)) to "Carbon dioxide"(CO_(2))`
In `CO_(2)` the element carbon and oxygen are combined as follows:
`underset(3g)underset(12g)(C)+underset(8g)underset(2xx16=32g)(2O) to underset(11g)underset(12+32=44g)(CO_(2))`
In the first case :
3.0 g of carbon are burnt in 8.0 g of oxygen to form 11.0 g of `CO_(2)`
In the second case:
3.0 g of carbon must be also combine with 8.0 g of oxgyen only. This meas that (50-8) - 42 g of oxgyen will remain unrecated.
The mass of `CO_(2)` in this case must be alos 11 g.