To a tank already containing N2 at 2.0 atm and O2 at 1.0 atm, we add an unknown quantity of CO2 until the total pressure is 4.6 atm. What is the partial pressure of the CO2?
See your post above.
To find the partial pressure of CO2 in the tank, we need to use Dalton's Law of Partial Pressure. According to Dalton's Law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas.
In this case, we have three gases in the tank: N2, O2, and CO2. The partial pressure of N2 is given as 2.0 atm, and the partial pressure of O2 is given as 1.0 atm. We need to find the partial pressure of CO2.
Let's denote the partial pressure of CO2 as P(CO2). According to Dalton's Law, the total pressure is the sum of the partial pressures:
Total pressure = P(N2) + P(O2) + P(CO2)
Given that the total pressure is 4.6 atm, the equation becomes:
4.6 atm = 2.0 atm + 1.0 atm + P(CO2)
To find the value of P(CO2), we rearrange the equation:
P(CO2) = 4.6 atm - 2.0 atm - 1.0 atm
= 1.6 atm
Therefore, the partial pressure of CO2 in the tank is 1.6 atm.