Question

two sealed, rigid 5.0 l containers each contain a gas at the same temperature but at a different pressure. nitrogen pressure = 1.0 atm oxygen + nitrogen pressure =? oxygen pressure = 0.8 atm 2 gases escape during the transfer of the entire contents of container 1 to container 2. assuming ideal behavior, which statement is correct regarding the total pressure of the gases after they are combined? a the total pressure of the gases in the mixture is the sum of the initial pressures because gas pressure only depends on the total amount of gas and temperature are held constant. b the total pressure of the gases in the mixture is lower than the sum of the initial because some of the energy of the particles will be lost due to an increase in the number of collisions. c the total pressure of the gases in the mixture is higher than the sum of the initial pressures of oxygen and nitrogen because of the intermolecular forces that develop between oxygen and nitrogen molecules. d the total pressure of the gases in the mixture cannot be determined because the actual value of the temperature is not given.

Explanation:

Step1: Recall Dalton's law of partial pressures

According to Dalton's law, for a mixture of non - reacting gases, the total pressure of a gas mixture is the sum of the partial pressures of the individual gases.

Step2: Calculate the total pressure

Given partial pressure of nitrogen ($P_{N_2}$) = 1.0 atm and partial pressure of oxygen ($P_{O_2}$)=0.8 atm. The total pressure ($P_{total}$) of the mixture of oxygen and nitrogen is $P_{total}=P_{N_2}+P_{O_2}$.
$P_{total}=1.0 + 0.8=1.8$ atm. And according to Dalton's law, the total pressure of the gases in the mixture in the new container is the sum of the initial pressures of nitrogen and oxygen gas because volume and temperature are held constant and the gases are assumed to be ideal (no intermolecular forces affecting the pressure in an ideal - gas scenario).

Answer:

A. The total pressure of the gases in the mixture is the sum of the initial pressures because pressure only depends on the total amount of gas and nitrogen and oxygen gas behave as ideal gases when volume and temperature are held constant.