Container A contains argon gas at 0C and pressure 380mmHg. Container B of volume 700 ml contains neon gas at 25C and pressure of 3atm. Both of these gases are placed in a 2L vessel at 273K and the total pressure is 1.46atm. What is the volume of container A?

Question

Container A contains argon gas at 0C and pressure 380mmHg. Container B of volume 700 ml contains neon gas at 25C and pressure of 3atm. Both of these gases are placed in a 2L vessel at 273K and the total pressure is 1.46atm. What is the volume of container A?

Answer 1

PV = nRT; solve for n = number mols Ar + Ne in the 2L vessel at the conditions listed.

PV = nRT in container B; solve for n = number of mols Ne.

Subtract total mols - mols Ne to give you mols Ar.

Then PV = nRT in container A; You have P, n, R, T; solve for V at the conditions listed.

Answer 2

To find the volume of container A, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Let's start by converting the given temperatures to Kelvin:
0°C + 273 = 273K (for argon gas)
25°C + 273 = 298K (for neon gas)
273K (for the final mixture)

Now let's consider the initial conditions of the gases in their separate containers:
Container A contains argon gas at 0°C (273 K) and a pressure of 380 mmHg. We need to convert the pressure to atm.
1 atm = 760 mmHg
380 mmHg / 760 mmHg = 0.5 atm

Container B contains neon gas at 25°C (298 K) and a pressure of 3 atm.

Now, let's calculate the number of moles of gas in each container using the ideal gas law equation. Since we're using the same volume for both gases in the final mixture, we can cancel out the volume factor:

For container A:
PV = nRT
(0.5 atm)(V) = (n)(0.0821 L·atm/mol·K)(273 K)
0.5V = 22.3833n

For container B:
(3 atm)(700 mL) = (n)(0.0821 L·atm/mol·K)(298 K)
2.1 = 24.4298n

Now, let's combine the gases in a 2L vessel at 273K (final mixture). The total pressure is given as 1.46 atm. We can use Dalton's Law of partial pressures to find the partial pressure of each gas in the mixture:

P_total = P_A + P_B

1.46 atm = P_A + P_B

Since P_A is 0.5 atm and P_B is 3 atm:

1.46 atm = 0.5 atm + 3 atm
1.46 atm = 3.5 atm

This equation cannot be satisfied because the sum of the partial pressures should equal the total pressure. Therefore, there might be an error in the given values or calculations.