how many moles of H2O will be produced from the complete combustion of 2.00g of CH4?
To determine the number of moles of H2O produced from the complete combustion of CH4, we need to use the balanced chemical equation for the reaction:
CH4 + 2O2 -> CO2 + 2H2O
From this equation, we can see that one mole of CH4 will produce 2 moles of H2O.
First, we need to find the number of moles of CH4 in 2.00g. To do this, we use the molar mass of CH4, which is 16.04 g/mol.
Number of moles of CH4 = Mass of CH4 / Molar mass of CH4
= 2.00g / 16.04 g/mol
= 0.124 moles
Since one mole of CH4 produces 2 moles of H2O, the number of moles of H2O produced can be calculated as follows:
Number of moles of H2O = Number of moles of CH4 × (2 moles of H2O / 1 mole of CH4)
= 0.124 moles × 2
= 0.248 moles
Therefore, the complete combustion of 2.00g of CH4 will produce 0.248 moles of H2O.
To determine the number of moles of H2O produced from the combustion of CH4, we need to use the balanced chemical equation for the reaction. The balanced equation for the combustion of CH4 is:
CH4 + 2O2 → CO2 + 2H2O
From this equation, we can see that for every 1 mole of CH4 combusted, 2 moles of H2O are produced.
To calculate the number of moles of H2O produced, we need to find the number of moles of CH4, given that we have 2.00g of CH4. To do this, we can use the molecular weight (molar mass) of CH4.
The molecular weight of CH4 is:
12.01 g/mol (C) + 4(1.01 g/mol) (4H) = 16.04 g/mol
Now, we can calculate the number of moles of CH4:
n(CH4) = mass/molecular weight
n(CH4) = 2.00g / 16.04 g/mol ≈ 0.1247 mol
Since the molar ratio is 1:2 (CH4:H2O), the number of moles of H2O produced is twice the number of moles of CH4:
n(H2O) = 2 × n(CH4) = 2 × 0.1247 mol = 0.2494 mol
Therefore, approximately 0.2494 moles of H2O will be produced from the complete combustion of 2.00g of CH4.