In the combustion of natural gas according to the equation CH4 + 2 O2 -> CO2 +2 H20, how many grams of water are formed during the combustion of 0.264 mole of CH4?

To determine the grams of water formed during the combustion of CH4, you need to use the given equation and the molar mass of water.

Step 1: Determine the molar mass of water (H2O):
The molar mass of hydrogen (H) is approximately 1 g/mol, and the molar mass of oxygen (O) is approximately 16 g/mol. Since there are two hydrogen atoms and one oxygen atom in water, the molar mass of water is:
(2 * 1 g/mol) + (1 * 16 g/mol) = 18 g/mol.

Step 2: Convert moles of CH4 to grams:
Given that you have 0.264 moles of CH4, you can multiply this by the molar mass of CH4 to convert to grams. The molar mass of CH4 (Carbon = 12 g/mol, Hydrogen = 1 g/mol) is:
(1 * 12 g/mol) + (4 * 1 g/mol) = 16 g/mol.
Therefore, the mass of 0.264 moles of CH4 is:
0.264 mol * 16 g/mol = 4.224 grams.

Step 3: Determine the moles of water produced:
According to the balanced equation, for every 1 mole of CH4 combusted, you will produce 2 moles of H2O. Therefore, you need to find the moles of water produced by multiplying the moles of CH4 by the stoichiometric coefficient for water.
0.264 mol CH4 * 2 mol H2O / 1 mol CH4 = 0.528 mol H2O.

Step 4: Convert the moles of water to grams:
Using the molar mass of water (18 g/mol) that was calculated earlier, you can convert moles of water to grams by multiplying by the molar mass.
0.528 mol H2O * 18 g/mol = 9.504 grams.

So, during the combustion of 0.264 moles of CH4, 9.504 grams of water are formed.

To determine the number of grams of water formed during the combustion of 0.264 moles of CH4, we need to use the molar mass and stoichiometry.

1. Determine the molar mass of water (H2O):
H: 1.00794 g/mol
O: 15.999 g/mol

Molar mass of H2O = 2(1.00794) + 15.999 = 18.015 g/mol

2. Use the stoichiometry to determine the number of moles of water formed:
From the balanced equation, the coefficient of CH4 (methane) is 1, and the coefficient of H2O (water) is 2.

Given moles of CH4 = 0.264 mol

According to the stoichiometry, 1 mole of CH4 produces 2 moles of H2O.

Therefore, moles of H2O = 0.264 mol CH4 x 2 mol H2O / 1 mol CH4 = 0.528 mol H2O

3. Convert the moles of water to grams:
Given moles of H2O = 0.528 mol H2O

Grams of H2O = moles of H2O x molar mass of H2O
= 0.528 mol H2O x 18.015 g/mol H2O
= 9.496 g H2O

So, during the combustion of 0.264 moles of CH4, 9.496 grams of water are formed.

0.264 mol CH4 will produce 2x that of H2O and convert mols to g. g H2O = molls H2O x molar mass H2O