A mixture of 25.0g of NO and an excess of O2 reacts according to the balanced equation. 2 NO + O2→2NO2. How many liters of NO2 are produced at STP?
To find out how many liters of NO2 are produced at STP, we need to use the given information regarding the mass of NO and the balanced equation.
Step 1: Calculate the number of moles of NO
To determine the number of moles of NO, we need to divide the given mass of NO (25.0g) by its molar mass. The molar mass of NO is 30.01 g/mol (14.01 g/mol for nitrogen + 16.00 g/mol for oxygen).
Moles of NO = Mass of NO / Molar mass of NO = 25.0g / 30.01 g/mol = 0.833 mol
Step 2: Use stoichiometry to relate NO to NO2
From the balanced equation, we see that 2 moles of NO react to produce 2 moles of NO2. This indicates a 1:1 mole ratio between NO and NO2.
Therefore, the number of moles of NO2 produced is also 0.833 mol.
Step 3: Convert moles of NO2 to volume at STP
At standard temperature and pressure (STP), one mole of any gas occupies 22.4 liters of volume.
Volume of NO2 at STP = Number of moles of NO2 * 22.4 L/mol = 0.833 mol * 22.4 L/mol = 18.64 L
Therefore, approximately 18.64 liters of NO2 are produced at STP when 25.0g of NO reacts with an excess of O2.