The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O₂(g) $\rightarrow$ 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

The oxidation of nitric oxide to nitrogen dioxide is 2NO(g) + O₂(g)

\rightarrow

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.

Quizplus · Accepted Answer

The balanced chemical equation is:2NO(g) + O₂(g) → 2NO₂(g)At STP, 100.0 mL of NO has a volume of 100.0 mL and a pressure of 1 atm. 400.0 mL of O₂ has a volume of 400.0 mL and a pressure of 1 atm.The total volume of the reaction mixture is 100.0 mL + 400.0 mL = 500.0 mL.The partial pressure of NO₂ in the final reaction mixture is:P_NO2 = (2 moles NO₂ / 500.0 mL) * (1 atm / 760 mmHg) = 0.222 atmTherefore, the correct answer is A.

The Oxidation of Nitric Oxide to Nitrogen Dioxide Is 2NO(g) →\rightarrow→

The Oxidation of Nitric Oxide to Nitrogen Dioxide Is 2NO(g) $\rightarrow$