Question

oxygen gas, contained in a 3.6 l vessel at 4.4 atm, is transferred to a 7.8 l vessel containing nitrogen at 1.7 atm. what is the total pressure in the 7.8 l vessel containing n2 and o2 gases? assume that there is no change in temperature. enter a pressure accurate to three significant figures.

Answer 1

To find the total pressure in the 7.8 L vessel containing N2 and O2 gases, you can calculate the partial pressure of the oxygen gas (O2) and then sum the partial pressures to find the total pressure. In this case, the total pressure is 3.60 atm.

Step-by-step explanation:

To find the total pressure in the 7.8 L vessel containing N2 and O2 gases, we can use the principles of partial pressure. We have the initial pressure of the oxygen gas (O2) in the 3.6 L vessel (4.4 atm) and the initial pressure of the nitrogen gas (N2) in the 7.8 L vessel (1.7 atm).

We can calculate the partial pressure of the oxygen gas (O2) using the formula P1V1 = P2V2, where P1 is the initial pressure of the oxygen gas, V1 is the initial volume of the oxygen gas, P2 is the final pressure of the oxygen gas, and V2 is the final volume of the oxygen gas.

Plugging in the values, we have (4.4 atm)(3.6 L) = P2(7.8 L). Solving for P2, we get a partial pressure of 1.90 atm for O2. The total pressure in the 7.8 L vessel containing N2 and O2 gases is the sum of the two resulting partial pressures: 1.90 atm + 1.70 atm = 3.60 atm. Therefore, the total pressure in the 7.8 L vessel is 3.60 atm.