CH4 + 202 + CO2 + 2H2O
How many grams of CO2 will be produced from 15.0 g of CH4 and 114 g of O2?

Mass =41.36 g

Explanation:

Given data:

Mass of CH₄ = 15 g

Mass of O₂ = 114 g

Mass of CO₂ produced = ?

Solution:

Chemical equation:

CH₄ + 2O₂    →  CO₂ + 2H₂O

Number of moles of CH₄:

Number of moles = mass/ molar mass

Number of moles = 15 g /16 g/mol

Number of moles = 0.94 mol

Number of moles of O₂:

Number of moles = mass/ molar mass

Number of moles = 114 g /32 g/mol

Number of moles = 3.6 mol

Now we will compare the moles of CO₂ with both reactant.

                            O₂             :            CO₂

                             2              :               1

                             3.6           :          1/2×3.6= 1.8 mol

                         CH₄              :            CO₂

                            1                :               1

                         0.94            :           0.94

Number of moles of CO₂ produced by CH₄ are less so it will limiting reactant.

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 0.94 mol × 44 g/mol

Mass =41.36 g

if you mean hydrogen and oxygen then water is the product

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