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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.
What is the correct pressure in kPa if the pressure is 1.54 ATM?
The correct pressure in kPa for 1.54 ATM is 156.6 kPa. This conversion is based on the fact that 1 ATM is equal to 101.3 kPa.
NO2 CO2 SO2 is in a bottle the partial pressure of NO2 is 1.25 atm and the partial pressure of CO2 is 2.63 atm if the total pressure of the gases is 11.20 atm what's the partial pressure of SO4?
The partial pressure of SO4 in a bottle of NO2, CO2, and SO2, is 7.32 atm.
A sample of helium gas has a volume of 900 milliliters and pressure of 2.50 ATM at 298k what is the new pressure when the temoerature is changed to 336 k and the volume is decreased to 450 milliliters?
Using the combined gas law, we can calculate the new pressure. The initial conditions are V1 = 900 mL, P1 = 2.50 ATM, and T1 = 298 K. The final conditions are V2 = 450 mL, T2 = 336 K. Using P1V1/T1 = P2V2/T2, we can solve for the new pressure, which is around 3.33 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.
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 0.23 ATM 0.42 ATM 0.89 ATM?
1.54 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.
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 will the total pressure be if two gases with pressure of 2 ATM and 3 ATM are mixed at a constant temperature?
2 atm + 3 atm
What is the total pressure of a gas mixture containing partial pressure of 0.23 ATM and 0.89 ATM?
1.54 atm
What is the total pressure of a gas mixture containing partial pressure of 0.23 ATM and 0.89 ATM.?
1.54 atm
