To find the moles of CO2 gas obtained at STP, we need to follow these steps:

Step 1: Determine the molar mass of CH4 (methane) and O2 (oxygen).
The molar mass of CH4 is calculated by adding up the atomic masses of each element in the compound. The atomic mass of carbon (C) is 12.01 g/mol, and the atomic mass of hydrogen (H) is 1.01 g/mol. Since methane has one carbon atom and four hydrogen atoms, the molar mass of CH4 is:
(1 * 12.01 g/mol) + (4 * 1.01 g/mol) = 16.05 g/mol

The molar mass of O2 is calculated by multiplying the atomic mass of oxygen (O) by 2, as there are two oxygen atoms in O2. The atomic mass of oxygen is 16.00 g/mol, so the molar mass of O2 is:
2 * 16.00 g/mol = 32.00 g/mol

Step 2: Calculate the moles of CH4 and O2.
To find the moles of a substance, we divide the given mass by its molar mass. In this case, we have 32 g of CH4 and 32 g of O2.

Moles of CH4 = 32 g / 16.05 g/mol = 1.993 mol
Moles of O2 = 32 g / 32.00 g/mol = 1.000 mol

Step 3: Determine the limiting reactant.
The limiting reactant is the reactant that is completely consumed in a chemical reaction, limiting the amount of product that can be formed. To find the limiting reactant, we compare the moles of each reactant to the stoichiometric ratio in the balanced chemical equation.

The balanced chemical equation for the reaction between CH4 and O2 to form CO2 is:
CH4 + 2O2 - CO2 + 2H2O

From the equation, we can see that 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2. Therefore, the stoichiometric ratio of CH4 to O2 is 1:2.

Since we have 1.993 moles of CH4 and 1.000 mole of O2, we can see that the moles of O2 are less than twice the moles of CH4. Therefore, O2 is the limiting reactant.

Step 4: Calculate the moles of CO2 produced.
Since O2 is the limiting reactant, we use its moles to determine the moles of CO2 produced. From the balanced chemical equation, we know that 1 mole of O2 produces 1 mole of CO2.

Moles of CO2 = Moles of O2 = 1.000 mol

Step 5: Convert moles of CO2 to volume at STP.
At STP (standard temperature and pressure), 1 mole of any ideal gas occupies 22.4 liters.

Volume of CO2 = Moles of CO2 * 22.4 L/mol
Volume of CO2 = 1.000 mol * 22.4 L/mol = 22.4 L

Therefore, the moles of CO2 gas obtained at STP when 32 g of CH4 reacted with 32 g of O2 is 1.000 mol, which is equivalent to 22.4 liters.

Question

To find the moles of CO2 gas obtained at STP, we need to follow these steps:

Step 1: Determine the molar mass of CH4 (methane) and O2 (oxygen).
The molar mass of CH4 is calculated by adding up the atomic masses of each element in the compound. The atomic mass of carbon (C) is 12.01 g/mol, and the atomic mass of hydrogen (H) is 1.01 g/mol. Since methane has one carbon atom and four hydrogen atoms, the molar mass of CH4 is:
(1 * 12.01 g/mol) + (4 * 1.01 g/mol) = 16.05 g/mol

The molar mass of O2 is calculated by multiplying the atomic mass of oxygen (O) by 2, as there are two oxygen atoms in O2. The atomic mass of oxygen is 16.00 g/mol, so the molar mass of O2 is:
2 * 16.00 g/mol = 32.00 g/mol

Step 2: Calculate the moles of CH4 and O2.
To find the moles of a substance, we divide the given mass by its molar mass. In this case, we have 32 g of CH4 and 32 g of O2.

Moles of CH4 = 32 g / 16.05 g/mol = 1.993 mol
Moles of O2 = 32 g / 32.00 g/mol = 1.000 mol

Step 3: Determine the limiting reactant.
The limiting reactant is the reactant that is completely consumed in a chemical reaction, limiting the amount of product that can be formed. To find the limiting reactant, we compare the moles of each reactant to the stoichiometric ratio in the balanced chemical equation.

The balanced chemical equation for the reaction between CH4 and O2 to form CO2 is:
CH4 + 2O2 -> CO2 + 2H2O

From the equation, we can see that 1 mole of CH4 reacts with 2 moles of O2 to produce 1 mole of CO2. Therefore, the stoichiometric ratio of CH4 to O2 is 1:2.

Since we have 1.993 moles of CH4 and 1.000 mole of O2, we can see that the moles of O2 are less than twice the moles of CH4. Therefore, O2 is the limiting reactant.

Step 4: Calculate the moles of CO2 produced.
Since O2 is the limiting reactant, we use its moles to determine the moles of CO2 produced. From the balanced chemical equation, we know that 1 mole of O2 produces 1 mole of CO2.

Moles of CO2 = Moles of O2 = 1.000 mol

Step 5: Convert moles of CO2 to volume at STP.
At STP (standard temperature and pressure), 1 mole of any ideal gas occupies 22.4 liters.

Volume of CO2 = Moles of CO2 * 22.4 L/mol
Volume of CO2 = 1.000 mol * 22.4 L/mol = 22.4 L

Therefore, the moles of CO2 gas obtained at STP when 32 g of CH4 reacted with 32 g of O2 is 1.000 mol, which is equivalent to 22.4 liters.

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