Calculate partial pressure Oxygen and nitric acid?

Question

Nitric oxide (NO) reacts with molecular oxygen as follows:
2NO(g) + O2(g) → 2NO2(g)
Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate their partial pressures. Assume that the temperatures remains constant at 25oC.
I couldn't add subscripts behind the elements, but the numbers behind them are suppose to be subscripts.

Nitric oxide (NO) reacts with molecular oxygen as follows:
2NO(g) + O2(g) → 2NO2(g)
Initially NO and O2 are separated as shown below. When the valve is opened, the reaction quickly goes to completion. Determine what gases remain at the end of the reaction and calculate their partial pressures. Assume that the temperatures remains constant at 25oC.
I couldn't add subscripts behind the elements, but the numbers behind them are suppose to be subscripts.

Volume of NO=2.00L
Pressure of No=3.00atm

Pressure of O2=4.00 atm
Volume of O2 = 3.00 L

Answer 1

All the NO will react, and 1/4 of the O2 will react.

NO2: 3 x 2/5 atm

O2: 3 x 3/5 atm.

Answer 2

which below plz?
You didn't give the initial amount of NO and O2 so the gases that remain cannot be calculated.
And NO2 is not nitric acid. Acid nitric is HNO3.