Carbon monoxide reacts with oxygen to form carbon dioxide.
2 CO(g) + O₂(g) $\to$ 2 CO₂(g)
In a 1.00 L flask,4.30 atm of CO reacts with 2.50 atm of O₂.Assuming that the temperature remains constant,what is the final pressure in the flask?

Question

Carbon monoxide reacts with oxygen to form carbon dioxide.
2 CO(g) + O₂(g)

\to

2 CO₂(g)
In a 1.00 L flask,4.30 atm of CO reacts with 2.50 atm of O₂.Assuming that the temperature remains constant,what is the final pressure in the flask?

Quizplus · Accepted Answer

According to the balanced equation, 2 moles of CO react with 1 mole of O2 to form 2 moles of CO2. Therefore, the moles of O2 required for the given amount of CO can be calculated as follows:

moles of CO = (pressure of CO) x (volume) / (RT) = (4.30 atm) x (1.00 L) / (0.0821 L atm/mol K) = 0.0524 mol

moles of O2 = 0.5 x (moles of CO) = 0.0262 mol

Since the moles of CO2 formed are also equal to the moles of O2 consumed, the final amount of CO2 can be calculated as follows:

moles of CO2 = 2 x (moles of O2) = 0.0524 mol

The final pressure can be calculated using the ideal gas law:

P = nRT / V = (0.0524 mol + 0.0262 mol) x (0.0821 L atm/mol K) x (298 K) / (1.00 L) = 4.65 atm

Therefore, the final pressure in the flask is 4.65 atm, which is answer choice D.

Carbon Monoxide Reacts with Oxygen to Form Carbon Dioxide →\to→ 2 CO2(g) in a 1

Carbon Monoxide Reacts with Oxygen to Form Carbon Dioxide $\to$ 2 CO₂(g)
in a 1