A student uses a pair of rigid bulbs connected by a tube of negligible volume. Initially, the stopcock between the bulbs is closed, and the conditions are shown in the table.

Bulb	Volume	Gas	Initial pressure	Initial temperature
A	\(1.00\ \text{L}\)	\(\text{H}_2\text{(g)}\)	\(4.00\ \text{atm}\)	\(600\ \text{K}\)
B	\(2.00\ \text{L}\)	\(\text{O}_2\text{(g)}\)	\(1.00\ \text{atm}\)	\(300\ \text{K}\)

The student opens the stopcock, allowing the gases to fill both bulbs, and then uses a spark to initiate the reaction

\[ 2\text{H}_2\text{(g)}+\text{O}_2\text{(g)}\rightarrow 2\text{H}_2\text{O(g)} \]

After the reaction is complete, the entire apparatus is maintained at \(600\ \text{K}\). At this temperature, all the water remains gaseous. Assuming ideal behavior, which of the following gives the final total pressure, \(P_{\text{total}}\), and the final partial pressure of \(\text{O}_2\), \(P_{\text{O}_2}\)?