What mass of water is produced from the complete combustion of 8.90×10−3g of methane
balance the equation
CH4+O2>>H2O + CO2
Then, when balanced, calculate the moles of methane you have (it won't be much, .0089g is a small quanitity).
Then,using the coefficents on the balanced equation, determine how many moles of water you get.
To find the mass of water produced from the complete combustion of methane, we need to determine the balanced chemical equation for the combustion of methane and then perform stoichiometric calculations.
The balanced chemical equation for the combustion of methane is:
CH₄ + 2O₂ → CO₂ + 2H₂O
From the equation, we can see that for every molecule of methane (CH₄) that reacts, two molecules of water (H₂O) are produced.
Now, let's calculate the number of methane molecules in 8.90×10−3g of methane using its molar mass.
The molar mass of methane (CH₄) is:
C: 12.01 g/mol
H: 1.008 g/mol
Molar mass of CH₄ = (12.01 * 1) + (1.008 * 4) = 16.04 g/mol
To calculate the number of moles of methane, we can use the formula:
Number of moles = Mass / Molar mass
Number of moles = 8.90×10−3g / 16.04 g/mol
Next, we can convert the moles of methane to moles of water using the stoichiometry of the balanced equation. From the equation, we know that the ratio of methane to water is 1:2.
So, the number of moles of water produced = Number of moles of methane * 2
After calculating the moles of water produced, we can convert it back to grams using the molar mass of water:
H: 1.008 g/mol
O: 16.00 g/mol
Molar mass of H₂O = (1.008 * 2) + (16.00 * 1) = 18.02 g/mol
Finally, we can find the mass of water produced by multiplying the number of moles of water by its molar mass:
Mass of water produced = Number of moles of water produced * Molar mass of water
By following these calculations, you should be able to find the mass of water produced from the complete combustion of 8.90×10−3g of methane.