We allow 24.0 g of CH4 to react as completely as possible with excess O2, to form CO2 and H2O . Write the balanced equation for this question . What mass of O2 reacts?

CH4 + 2O2 ==> CO2 + 2H2O

mols CH4 = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols CH4 to mols O2.
Then g O2 = mols O2 x molar mass O2 = ?

24.0g CH4 * 1mol CH4/16.04gCH4 * 1mol O2/1molCH4 = 1.5 MOL O2

To write the balanced equation, we need to know the chemical formulas of the reactants and products involved.

For this question, methane (CH4) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).

The balanced equation for this reaction is:

CH4 + 2O2 -> CO2 + 2H2O

According to the balanced equation, 1 mole of CH4 reacts with 2 moles of O2 to form 1 mole of CO2 and 2 moles of H2O.

To determine the mass of O2 that reacts, we need to know the molar mass of CH4. The molar mass of carbon (C) is 12.01 g/mol, and the molar mass of hydrogen (H) is 1.01 g/mol.

The molar mass of CH4:

12.01 g/mol (for carbon) + (4 x 1.01 g/mol) (for hydrogen) = 16.05 g/mol

Since we have 24.0 g of CH4, we can calculate the number of moles of CH4:

Moles of CH4 = Mass of CH4 / Molar mass of CH4
Moles of CH4 = 24.0 g / 16.05 g/mol
Moles of CH4 ≈ 1.49 mol

According to the balanced equation, 1 mole of CH4 reacts with 2 moles of O2. Therefore, the number of moles of O2 required for the reaction is:

Moles of O2 = 2 x Moles of CH4
Moles of O2 = 2 x 1.49 mol
Moles of O2 ≈ 2.98 mol

Lastly, to determine the mass of O2 that reacts, we need to know the molar mass of O2. The molar mass of oxygen (O) is 16.00 g/mol.

The mass of O2:

Mass of O2 = Moles of O2 x Molar mass of O2
Mass of O2 = 2.98 mol x 16.00 g/mol
Mass of O2 ≈ 47.7 g

So, approximately 47.7 grams of O2 will react with 24.0 grams of CH4.

To write the balanced equation for the reaction between CH4 (methane) and O2 (oxygen), we need to determine the stoichiometric coefficients that balance the number of atoms on both sides of the equation.

The combustion of methane can be represented by the following balanced equation:

CH4 + 2O2 → CO2 + 2H2O

In this equation, one molecule of CH4 reacts with two molecules of O2 to produce one molecule of CO2 and two molecules of H2O.

Now, to find the mass of O2 that reacts, we can use the stoichiometry of the balanced equation.

1 mole of CH4 (molar mass 16.04 g/mol) reacts with 2 moles of O2 (molar mass 32.00 g/mol). This means that the mole ratio of CH4 to O2 is 1:2.

Given the mass of CH4 as 24.0 g, we can convert it to moles by dividing the mass by the molar mass:

24.0 g CH4 * (1 mol CH4 / 16.04 g CH4) = 1.496 moles CH4

Since the mole ratio of CH4 to O2 is 1:2, we can calculate the moles of O2 required:

1.496 moles CH4 * (2 moles O2 / 1 mol CH4) = 2.992 moles O2

Finally, we can convert the moles of O2 back to mass using the molar mass:

2.992 moles O2 * (32.00 g O2 / 1 mol O2) = 95.744 g O2

Therefore, 95.744 grams of O2 will react with 24.0 grams of CH4 to form CO2 and H2O.