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To solve for atmospheric pressure (ATM) in a given context, you typically use the formula relating pressure, volume, and temperature, commonly derived from the ideal gas law: ( PV = nRT ). Here, ( P ) stands for pressure, ( V ) for volume, ( n ) for the number of moles, ( R ) for the ideal gas constant, and ( T ) for temperature in Kelvin. If you're measuring atmospheric pressure, you can also use a barometer or pressure gauge to obtain the value directly. Standard atmospheric pressure at sea level is about 101.3 kPa or 760 mmHg.
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A mixture of He Ne and N2 gases has a pressure of 1.943 ATM. If the pressures of He and Ne are 0.137 ATM and 0.566 ATM respectively what is the partial pressure of N2 in the mixture?
To find the partial pressure of N2 in the mixture, we 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. Given the total pressure (1.943 ATM) and the partial pressures of He (0.137 ATM) and Ne (0.566 ATM), we can calculate the partial pressure of N2 as follows: Partial pressure of N2 = Total pressure - (Partial pressure of He + Partial pressure of Ne) Partial pressure of N2 = 1.943 ATM - (0.137 ATM + 0.566 ATM) = 1.943 ATM - 0.703 ATM = 1.240 ATM. So, the partial pressure of N2 is 1.240 ATM.
What is the total pressure of a gas mixture containing partial pressure of ATM and 089 ATM?
To find the total pressure of a gas mixture, you simply add the partial pressures of the individual gases. In this case, if one gas has a partial pressure of 1 ATM and another has a partial pressure of 0.89 ATM, the total pressure would be 1 ATM + 0.89 ATM = 1.89 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.
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.
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.
If i have 5.6liters of gas in a piston at a pressure of 1.5 ATM and compress the gas volume is 4.8L what will the new pressure be?
To find the new pressure, we can use Boyle's Law, which states that pressure and volume are inversely proportional at constant temperature. By applying the formula P1V1 = P2V2, where P1 = 1.5 ATM, V1 = 5.6 L, and V2 = 4.8 L, we can solve for P2. Thus, the new pressure would be 1.75 ATM.
A 2.0 liter container of nitrogen had a pressure of 3.2 ATM what volume would be necessary to decrease the pressure to 1.0atm?
To decrease the pressure of the nitrogen to 1.0 atm, you would need to increase the volume. Use the combined gas law (P1V1/T1 = P2V2/T2) to calculate the new volume required. Given that the initial pressure is 3.2 atm, initial volume is 2.0 liters, and final pressure is 1.0 atm, you can rearrange the equation to solve for V2.
1.00 L of a gas at standard temperature and pressure is compressed to 473 mL What is the new pressure of the gas?
Using the ideal gas law, we can calculate the new pressure of the gas. The initial pressure is 1 atm, the initial volume is 1.00 L, and the final volume is 0.473 L. By applying the formula P1V1 = P2V2, we can solve for the new pressure of the gas after compression.
A mixture of He Ne and N2 gases has a pressure of 1.943 ATM. If the pressures of He and Ne are 0.137 ATM and 0.566 ATM respectively what is the partial pressure of N2 in the mixture?
To find the partial pressure of N2 in the mixture, we 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. Given the total pressure (1.943 ATM) and the partial pressures of He (0.137 ATM) and Ne (0.566 ATM), we can calculate the partial pressure of N2 as follows: Partial pressure of N2 = Total pressure - (Partial pressure of He + Partial pressure of Ne) Partial pressure of N2 = 1.943 ATM - (0.137 ATM + 0.566 ATM) = 1.943 ATM - 0.703 ATM = 1.240 ATM. So, the partial pressure of N2 is 1.240 ATM.
What will the total pressure be and partial pressure be if two gases with pressures of 2 ATM and 3 ATM are mixed at a constant temperature?
The total pressure of the mixed gases will be 5 ATM. The partial pressure of each gas will remain the same as their individual pressures before mixing, so the partial pressure for the gas originally at 2 ATM will remain at 2 ATM, and the gas originally at 3 ATM will remain at 3 ATM.
What is the total pressure of a gas mixture containing partial pressure of 0.23 ATM 0.42 ATM 0.89 ATM?
1.54 atm
What is the total pressure of a gas mixture containing partial pressure of 0.23 ATM 0.42 ATM and 0.89 ATM?
1.54 atm
What is the total pressure of a gas mixture containing partial pressure of ATM and 089 ATM?
To find the total pressure of a gas mixture, you simply add the partial pressures of the individual gases. In this case, if one gas has a partial pressure of 1 ATM and another has a partial pressure of 0.89 ATM, the total pressure would be 1 ATM + 0.89 ATM = 1.89 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.
What is the total pressure of a gas mixture containing partial pressure of .23 ATM .42 ATM and .89 ATM?
1.54atm
What change in pressure would result in the volume of gas increasing A 2 ATM to 3 ATM B 3 ATM to 4 ATM C 4 ATM to 1 ATM D 1 ATM to 3 ATM?
A. An increase in pressure from 2 ATM to 3 ATM will result in a decrease in volume of gas. B. An increase in pressure from 3 ATM to 4 ATM will result in a decrease in volume of gas. C. A decrease in pressure from 4 ATM to 1 ATM will result in an increase in volume of gas. D. An increase in pressure from 1 ATM to 3 ATM will result in a decrease in volume of gas.
What is the total pressure of a gas mixture containing partial pressure of 0.23 ATM and 0.89 ATM?
1.54 atm
