The following reaction consumes 2.40 kg of CO, How many total liters of gas are formed at STP?

Here is a stoichiometry problem I've posted. Just follow the steps remembering 1 mole gas occupies 22.4 L at STP.

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To find the number of liters of gas formed at STP, we need to first determine the number of moles of CO that react and then use the ideal gas law to convert moles into liters.

Step 1: Find the number of moles of CO.
To do this, we need to know the molar mass of CO, which is the sum of the atomic masses of carbon (12.01 g/mol) and oxygen (16.00 g/mol).
The molar mass of CO = 12.01 g/mol + 16.00 g/mol = 28.01 g/mol.

Next, we convert the given mass of CO (2.40 kg) into grams.
The mass of CO = 2.40 kg * 1000 g/kg = 2400 g.

Now, we can calculate the number of moles of CO.
Number of moles = given mass / molar mass = 2400 g / 28.01 g/mol ≈ 85.68 mol.

Step 2: Convert moles of CO into liters of gas at STP.
According to the ideal gas law, 1 mole of any gas occupies 22.4 liters at standard temperature and pressure (STP).

Therefore, the total volume of gas formed can be calculated by multiplying the number of moles of CO by the molar volume at STP.
Total volume = Number of moles * Molar volume = 85.68 mol * 22.4 L/mol ≈ 1918.59 L.

So, the total liters of gas formed at STP in this reaction is approximately 1918.59 L.