The oxidation of nitric oxide to nitrogen dioxide is
2NO(g) + O₂(g) → 2NO₂(g)
If 100.0 mL of NO (at STP) reacts with 400.0 mL of O₂ at STP, calculate the partial pressure of NO₂ in the final reaction mixture.

Question

Quizplus · Accepted Answer

The correct answer is A because the partial pressure of NO2 in the final reaction mixture is 0.222 atm. This can be calculated using the ideal gas law, which states that the partial pressure of a gas is equal to the number of moles of that gas divided by the total volume of the gas. In this case, the number of moles of NO2 is equal to the number of moles of NO that reacted, which is 100.0 mL / 22.4 L/mol = 0.00446 mol. The total volume of the gas is equal to the sum of the volumes of NO and O2, which is 100.0 mL + 400.0 mL = 500.0 mL. Therefore, the partial pressure of NO2 is 0.00446 mol / 0.5 L = 0.222 atm.

The Oxidation of Nitric Oxide to Nitrogen Dioxide Is