Sure, here's how to solve this problem:

Step 1: First, we need to find the total initial pressure in the 5.2 L canister. This is the sum of the pressures of nitrogen and xenon, which is 125 kPa + 147.8 kPa = 272.8 kPa.

Step 2: The total volume after the 5.2 L canister is attached to the 6.2 L canister is 5.2 L + 6.2 L = 11.4 L.

Step 3: We can use the ideal gas law, which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume. In this case, the initial pressure and volume are 272.8 kPa and 5.2 L, and the final volume is 11.4 L. We can set up the equation as follows:

P1*V1 = P2*V2

where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.

Step 4: Solving for P2, we get:

P2 = P1*V1/V2 = 272.8 kPa * 5.2 L / 11.4 L = 124.4 kPa

So, the final pressure of the gaseous mixture is 124.4 kPa.

Question

Sure, here's how to solve this problem:

Step 1: First, we need to find the total initial pressure in the 5.2 L canister. This is the sum of the pressures of nitrogen and xenon, which is 125 kPa + 147.8 kPa = 272.8 kPa.

Step 2: The total volume after the 5.2 L canister is attached to the 6.2 L canister is 5.2 L + 6.2 L = 11.4 L.

Step 3: We can use the ideal gas law, which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume. In this case, the initial pressure and volume are 272.8 kPa and 5.2 L, and the final volume is 11.4 L. We can set up the equation as follows:

P1*V1 = P2*V2

where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.

Step 4: Solving for P2, we get:

P2 = P1*V1/V2 = 272.8 kPa * 5.2 L / 11.4 L = 124.4 kPa

So, the final pressure of the gaseous mixture is 124.4 kPa.

Knowee AI · Accepted Answer

Sure, here's how to solve this problem:

Step 1: First, we need to find the total initial pressure in the 5.2 L canister. This is the sum of the pressures of nitrogen and xenon, which is 125 kPa + 147.8 kPa = 272.8 kPa.

Step 2: The total volume after the 5.2 L canister is attached to the 6.2 L canister is 5.2 L + 6.2 L = 11.4 L.

Step 3: We can use the ideal gas law, which states that the product of the initial pressure and volume is equal to the product of the final pressure and volume. In this case, the initial pressure and volume are 272.8 kPa and 5.2 L, and the final volume is 11.4 L. We can set up the equation as follows:

P1*V1 = P2*V2

where P1 is the initial pressure, V1 is the initial volume, P2 is the final pressure, and V2 is the final volume.

Step 4: Solving for P2, we get:

P2 = P1*V1/V2 = 272.8 kPa * 5.2 L / 11.4 L = 124.4 kPa

So, the final pressure of the gaseous mixture is 124.4 kPa.

A 5.2 L cannister contains nitrogen at 125 kPa and xenon at 147.8 kPa. When this cannister, is attached to another evacuated cannister that is 6.2 litres in size, what is the final pressure of the gaseous mixture.

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