For the reaction
CH4+ 2 O2 → CO2+ 2 H2O ,
what is the maximum amount of CO2
(44.0095 g/mol) which could be formed from
15.3 g of CH4 (16.0425 g/mol) and 6.2 g of O2
(31.9988 g/mol)?
Answer in units of g
To find the maximum amount of CO2 that can be formed in the reaction, we need to determine the limiting reactant. The limiting reactant is the reactant that is completely consumed and determines the maximum amount of product that can be formed.
First, we need to calculate the number of moles of CH4 and O2:
Number of moles of CH4 = mass of CH4 / molar mass of CH4
Number of moles of CH4 = 15.3 g / 16.0425 g/mol = 0.955 mol
Number of moles of O2 = mass of O2 / molar mass of O2
Number of moles of O2 = 6.2 g / 31.9988 g/mol = 0.194 mol
Next, we will use the balanced equation to determine the stoichiometry between CH4 and CO2. From the balanced equation, we can see that 1 mole of CH4 reacts to produce 1 mole of CO2.
Therefore, the number of moles of CO2 that can be formed from CH4 = 0.955 mol.
Finally, we can calculate the mass of CO2 using the number of moles and the molar mass of CO2:
Mass of CO2 = number of moles of CO2 * molar mass of CO2
Mass of CO2 = 0.955 mol * 44.0095 g/mol = 41.98 g
Therefore, the maximum amount of CO2 that could be formed from 15.3 g of CH4 and 6.2 g of O2 is 41.98 grams.