What mass of CO2 could be formed from the reaction of 16 g of CH4 with 32 g of O2 ?
Here is a worked example of a stoichiometry problem. http://www.jiskha.com/science/chemistry/stoichiometry.html
C H4 + 2 O2 --> CO2 + 2H2O
C is 12 g/mol
CH4 is 16 g/mol so we have one mol
O is 16 g/mol
O2 is 32 g/mol
so we have one mole but we need 2
so
Only half a mole of CH4 reacts with the one mole of O2
That is 6 grams of C with 16 of our 32 grams of O
so 6 + 16 = 22 grams of CO2
To determine the mass of CO2 formed from the reaction of CH4 with O2, we need to use the balanced chemical equation for the reaction:
CH4 + 2O2 -> CO2 + 2H2O
The balanced equation tells us that one molecule of CH4 reacts with two molecules of O2 to produce one molecule of CO2 and two molecules of H2O.
Let's calculate the number of moles of CH4 and O2:
Molar mass of CH4 (carbon dioxide): 12.01 g/mol + 4(1.01 g/mol) = 16.05 g/mol
Molar mass of O2 (oxygen gas): 2(16 g/mol) = 32 g/mol
Number of moles of CH4 = mass / molar mass = 16 g / 16.05 g/mol = 0.996 moles
Number of moles of O2 = mass / molar mass = 32 g / 32 g/mol = 1.0 mole
According to the balanced equation, the ratio between CH4 and CO2 is 1:1. Therefore, the number of moles of CO2 formed will also be 0.996 moles.
Now, let's calculate the mass of CO2 formed:
Molar mass of CO2 (carbon dioxide): 12.01 g/mol + 2(16 g/mol) = 44.01 g/mol
Mass of CO2 formed = number of moles x molar mass = 0.996 moles x 44.01 g/mol = 43.79 grams
Therefore, the mass of CO2 formed from the reaction of 16 g of CH4 with 32 g of O2 is approximately 43.79 grams.