if 6.00g of CH4 was completely combusted in 15.00g of O2. How much H2O and CO2 will be produced?

To determine the amount of H2O and CO2 produced when 6.00g of CH4 (methane) is combusted with 15.00g of O2 (oxygen), we first need to balance the combustion equation for CH4.

The balanced equation for the combustion of methane can be written as follows:
CH4 + 2O2 → CO2 + 2H2O

From the balanced equation, we can see that 1 molecule of CH4 reacts with 2 molecules of O2 to produce 1 molecule of CO2 and 2 molecules of H2O.

Now, let's calculate the amount of CO2 produced:
- First, calculate the molar mass of CH4 (methane):
Molar mass of CH4 = 12.01g/mol (C) + 4 * 1.01g/mol (H) = 16.05g/mol

- Use the molar mass of CH4 to convert the given mass (6.00g) to moles:
moles of CH4 = 6.00g / 16.05g/mol ≈ 0.373 mol

Since the mole ratio between CH4 and CO2 is 1:1, the amount of CO2 produced will also be 0.373 mol.

- Calculate the molar mass of CO2 (carbon dioxide):
Molar mass of CO2 = 12.01g/mol (C) + 2 * 16.00g/mol (O) = 44.01g/mol

- Use the molar mass of CO2 to convert the moles of CO2 to grams:
mass of CO2 = 0.373 mol * 44.01g/mol ≈ 16.40g

Therefore, approximately 16.40g of CO2 will be produced.

Now, let's calculate the amount of H2O produced:
- Since the mole ratio between CH4 and H2O is 1:2, the number of moles of H2O produced will be twice the moles of CH4.

moles of H2O = 2 * moles of CH4 = 2 * 0.373 mol = 0.746 mol

- Calculate the molar mass of H2O (water):
Molar mass of H2O = 2 * 1.01g/mol (H) + 16.00g/mol (O) = 18.02g/mol

- Use the molar mass of H2O to convert the moles of H2O to grams:
mass of H2O = 0.746 mol * 18.02g/mol ≈ 13.42g

Therefore, approximately 13.42g of H2O will be produced.

In summary, the combustion of 6.00g of CH4 with 15.00g of O2 will produce approximately 16.40g of CO2 and 13.42g of H2O.