What mass of oxygen is needed for the complete combustion of 5.00×10−3g of methane?
To determine the mass of oxygen needed for the complete combustion of methane, we first need to balance the chemical equation for the combustion reaction. The balanced equation for the combustion of methane (CH4) is:
CH4 + 2O2 → CO2 + 2H2O
From the balanced equation, we can see that for every one molecule of methane, we need two molecules of oxygen.
Now, let's calculate the molar mass of methane (CH4) and oxygen (O2):
Molar mass of CH4:
C = 12.01 g/mol
H = 1.008 g/mol (x4)
Total molar mass of CH4 = 16.04 g/mol
Molar mass of O2:
O = 16.00 g/mol (x2)
Total molar mass of O2 = 32.00 g/mol
Next, we need to convert the given mass of methane (5.00x10^-3 g) to moles:
Moles of CH4 = Mass / Molar mass
Moles of CH4 = 5.00x10^-3 g / 16.04 g/mol
Moles of CH4 ≈ 0.0003116 mol
Using the balanced equation, we know that the mole ratio between CH4 and O2 is 1:2. Therefore, the moles of O2 needed for complete combustion would be twice the moles of CH4:
Moles of O2 = 2 × Moles of CH4
Moles of O2 = 2 × 0.0003116 mol
Moles of O2 ≈ 0.0006232 mol
Finally, we can calculate the mass of oxygen needed by multiplying the moles of O2 by its molar mass:
Mass of O2 = Moles of O2 × Molar mass of O2
Mass of O2 = 0.0006232 mol × 32.00 g/mol
Mass of O2 ≈ 0.0199 g
Therefore, approximately 0.0199 grams of oxygen is needed for the complete combustion of 5.00 × 10^-3 grams of methane.
To determine the mass of oxygen needed for the complete combustion of methane, we need to balance the chemical equation for the combustion reaction.
The combustion of methane (CH4) can be represented by the balanced equation:
CH4 + 2O2 → CO2 + 2H2O
From the balanced equation, we can see that for every 1 mole of methane (CH4) combusted, we need 2 moles of oxygen (O2). Thus, we need to find the molar amount of methane in order to determine the amount of oxygen required.
First, we need to convert the given mass of methane (5.00×10−3g) to moles. To do this, we need to know the molar mass of methane, which is 16.04 g/mol.
Moles of CH4 = (Given mass of CH4) / (Molar mass of CH4)
= 5.00×10−3 g / 16.04 g/mol
Now that we know the moles of CH4, we can determine the moles of O2 required by using the stoichiometric ratio from the balanced equation (1 mole CH4: 2 moles O2).
Moles of O2 required = (Moles of CH4) x (2 moles O2 / 1 mole CH4)
Finally, to find the mass of oxygen required, we multiply the moles of O2 by the molar mass of oxygen, which is 32.00 g/mol.
Mass of O2 required = (Moles of O2 required) x (Molar mass of O2)
By following these steps and plugging in the values, you should be able to calculate the mass of oxygen needed for the complete combustion of the given mass of methane.
The balanced equation follows:
CH4 2O2 ==> CO2 + 2H2O
Now follow the guidelines from the NH3 post. Same procedure.