Final answer:
The final pressure of a mixture of gases can be determined using Dalton's Law of Partial Pressures, and by adding the pressures of the individual gases and adjusting for the total volume. In this case, the final combined pressure is 426 torr, which is option (a).
Step-by-step explanation:
To determine the final pressure when two gases mix in a combined volume, without any temperature change, we can use Dalton's Law of Partial Pressures. According to this law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. Since both bulbs are 1.00 L and the gases are at the same temperature, we can simply add the pressures.
The pressure of oxygen gas is 424 torr, and the pressure of hydrogen gas is 428 torr. The total final pressure is the sum of these two pressures:
Final pressure = Pressure of O2 + Pressure of H2
Final pressure = 424 torr + 428 torr
Final pressure = 852 torr
However, because the gases are now occupying a combined volume of 2.00 L (1.00 L + 1.00 L), we have to account for the doubled volume. So the final pressure per liter would be halved:
Final pressure (per liter) = 852 torr / 2
Final pressure (per liter) = 426 torr
Therefore, the correct answer is that the final pressure in the system is 426 torr, which corresponds to option (a).