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What is the pressure inside a container if it contains Ne gas at a pressure of 2.0 ATM He gas at a pressure of 1.5 ATM and N2 gas at a pressure of 2.5 ATM?
To find the total pressure inside the container, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of the individual gases. Therefore, the total pressure would be 2.0 ATM (Ne) + 1.5 ATM (He) + 2.5 ATM (N2) = 6.0 ATM. Thus, the pressure inside the container is 6.0 ATM.
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A pressurized tank contains a mixture of oxygen and helium.if the partial pressure of oxygen is 10atm and the partial pressure of helium is 32.8 ATM what is the total pressure inside the tank?
The total pressure inside the tank is the sum of the partial pressures of the gases present. In this case, Total pressure = partial pressure of oxygen + partial pressure of helium = 10 atm + 32.8 atm = 42.8 atm.
The pressure of a sample of helium in a 1.00 L container is 0.988 ATM What is the new pressure if the sample is placed in a 4.40 L container?
The pressure of the helium will decrease when placed in the larger container, following Boyle's Law. Using the formula P1V1 = P2V2, we can calculate the new pressure. So, (0.988 ATM)(1.00 L) = P2(4.40 L), which gives P2 = 0.225 ATM.
A tank contains N2 at 1.0 ATM and O2 at 2.0 ATM Helium is added to this tank until the total pressure is 6.0 ATM What is the partial pressure of the helium?
The initial total pressure is 1.0 ATM + 2.0 ATM = 3.0 ATM. Therefore, 6.0 ATM - 3.0 ATM = 3.0 ATM of helium was added to the tank. Hence, the partial pressure of helium in the tank is 3.0 ATM.
Suppose two gases in a container have a total pressure of 1.20 ATM. What is the pressure of gas b if the partial of gas a is 0.75 ATM?
To find the pressure of gas B, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of individual gases. Given that the total pressure is 1.20 ATM and the partial pressure of gas A is 0.75 ATM, you can calculate the pressure of gas B as follows: Pressure of gas B = Total pressure - Pressure of gas A = 1.20 ATM - 0.75 ATM = 0.45 ATM. Thus, the pressure of gas B is 0.45 ATM.
When a container is filled with 3 moles of H 2 moles of O and 1 mole of N the pressure in the container is 8.7 ATM. The partial pressure of O 2 is?
impossible to calculate
A pressurized tank contains a mixture of oxygen and helium If the partial pressure of oxygen is 10 atm and the partial pressure of helium is 32.8 atm what is the total pressure inside the tank?
42.8 atm fufurjthfhhudjd
A pressurized tank contains a mixture of oxygen and helium.if the partial pressure of oxygen is 10atm and the partial pressure of helium is 32.8 ATM what is the total pressure inside the tank?
The total pressure inside the tank is the sum of the partial pressures of the gases present. In this case, Total pressure = partial pressure of oxygen + partial pressure of helium = 10 atm + 32.8 atm = 42.8 atm.
The pressure of a sample of helium in a 1.00 L container is 0.988 ATM What is the new pressure if the sample is placed in a 4.40 L container?
The pressure of the helium will decrease when placed in the larger container, following Boyle's Law. Using the formula P1V1 = P2V2, we can calculate the new pressure. So, (0.988 ATM)(1.00 L) = P2(4.40 L), which gives P2 = 0.225 ATM.
A tank contains N2 at 1.0 ATM and O2 at 2.0 ATM Helium is added to this tank until the total pressure is 6.0 ATM What is the partial pressure of the helium?
The initial total pressure is 1.0 ATM + 2.0 ATM = 3.0 ATM. Therefore, 6.0 ATM - 3.0 ATM = 3.0 ATM of helium was added to the tank. Hence, the partial pressure of helium in the tank is 3.0 ATM.
Suppose two gases in a container have a total pressure of 1.20 ATM. What is the pressure of gas b if the partial of gas a is 0.75 ATM?
To find the pressure of gas B, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of individual gases. Given that the total pressure is 1.20 ATM and the partial pressure of gas A is 0.75 ATM, you can calculate the pressure of gas B as follows: Pressure of gas B = Total pressure - Pressure of gas A = 1.20 ATM - 0.75 ATM = 0.45 ATM. Thus, the pressure of gas B is 0.45 ATM.
The pressure inside a hydrogen filled container was 2.10 ATM ta 21 degrees Celsius what would the pressure be if the container was heated to 99 degrees Celsius?
To find the new pressure, we can use the combined gas law which states P1/T1 = P2/T2. Plugging in the values: P1 = 2.10 ATM, T1 = 21°C + 273 = 294 K, T2 = 99°C + 273 = 372 K, we can solve for P2. The new pressure would be approximately 2.80 ATM.
Suppose two gases in a container have a total pressure of 1.20atm what is the pressure of gas B if the partial pressure of gas A is 0.75atm?
The pressure of gas B can be calculated by subtracting the partial pressure of gas A from the total pressure. Therefore, the pressure of gas B would be 1.20 atm - 0.75 atm = 0.45 atm.
How do an ATM read an ATM pin?
ATM card readers built inside the ATM machines can read the magnetic strip that contains every information about the ATM card including the PIN number.
When a container is filled with 3 moles of H 2 moles of O and 1 mole of N the pressure in the container is 8.7 ATM. The partial pressure of O 2 is?
impossible to calculate
How Many Moles of air are there in a 3 L container of 1 ATM pressure and 293?
0.125 moles
How many moles are there in a 3 L container at 1 ATM pressure and 293 K?
The answer is 0,125 moles.
When a container is filled with 3 moles of H½ 2 moles of O½ and 1 mole of N½ the pressure in the container is 8.7 atm The partial pressure of O½ is?
To find the partial pressure of O₂, we need to calculate its mole fraction in the mixture. The total moles in the container is 3 + 2 + 1 = 6 moles. The mole fraction of O₂ is 2/6 = 1/3. As the total pressure is 8.7 atm, the partial pressure of O₂ is the mole fraction of O₂ multiplied by the total pressure, giving 1/3 * 8.7 = 2.9 atm.
