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What volume of oxygen gas at 320k and 680 torr will react with 2.50 L?
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∙ 14y ago
To determine the volume of oxygen gas required, we first need to convert the temperature to Kelvin (320 K) and pressure to atm (680 torr = 0.895 atm). Then, we can use the ideal gas law equation, V = nRT/P, where n is the number of moles, R is the ideal gas constant, and V is the volume. Calculate the number of moles using the given volume and pressure, then rearrange the equation to solve for the volume of oxygen gas needed.
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What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure when temperature is constant. So, if the pressure increases from 740 Torr to 780 Torr, the volume will decrease accordingly. Using the formula P1V1 = P2V2, where P1 = 740 Torr, V1 = 500 ml, and P2 = 780 Torr, you can solve for V2 to find the final volume.
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
To find the final pressure of the nitrogen, we can use Boyle's Law which states that the pressure and volume of a gas are inversely proportional when temperature is constant. Therefore, 100 mL * 810 torr = 72 mL * final pressure. Solving for final pressure, we get: final pressure = (100 mL * 810 torr) / 72 mL = 1125 torr. So, the pressure of the trapped nitrogen in the syringe is 1125 torr.
a gas has a pressure of 766.7 torr at a temperature of 10.0°C. the sample contains 2.35 moles of xenon. what is the volume of the gas in liters?
Using PV=nRT, 10.0ºC = 283.15ºK, R = 62.36 L torr/mol K V= (nRT)/P V = (2.35m*(62.36 L torr/mol K)*283.15ºK)/766.7 Torr V = 54.12 L
What is the partial pressure of N2 and O2 having a total pressure of 1075 torr if the partial pressure of 02 is 720 torr?
1075 torr - 720 torr = 355 torr
The temperature of a gas in a sealed container changes from 20.0C to 40.0C if the volume remains constant the pressure will change from 660 torr to?
Using Charles's Law (V1/T1 = V2/T2), we can find the new pressure which would be approximately 720 torr when the temperature increases from 20.0C to 40.0C while keeping the volume constant.
What is the volumeof one mole of oxygen gas at 273 K and 760 torr?
The volume of one mole of any ideal gas at standard temperature and pressure (273 K and 1 atm) is approximately 22.4 L. Since the pressure given is 760 torr, which is equivalent to 1 atm, the volume of one mole of oxygen gas at 273 K and 760 torr would also be approximately 22.4 L.
What will be the final volume of a 500 ml sample of helium if its pressure is changed from 740 Torr to 780 Torr and its temperature is kept constant?
According to Boyle's Law, the volume of a gas is inversely proportional to its pressure when temperature is constant. So, if the pressure increases from 740 Torr to 780 Torr, the volume will decrease accordingly. Using the formula P1V1 = P2V2, where P1 = 740 Torr, V1 = 500 ml, and P2 = 780 Torr, you can solve for V2 to find the final volume.
A 110.0 mL sample of nitrogen at 820 torr was compressed to a volume of 83.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
Using Boyle's law (P1V1 = P2V2), the initial pressure is 820 torr, the initial volume is 110.0 mL, and the final volume is 83.0 mL. Solving for P2, we get P2 = (P1V1) / V2 = (820 torr * 110.0 mL) / 83.0 mL = 1088.55 torr. Therefore, the pressure of the trapped nitrogen in the syringe is 1088.55 torr.
What volume will oxygen gas that occupies a volume of 250 ml at 740 torr pressure occupy at 800 torr pressure?
Using Boyle's Law (P1V1 = P2V2), the initial pressure, volume, and new pressure are given. Rearranging the formula to solve for V2: V2 = (P1 * V1) / P2 = (740 torr * 250 ml) / 800 torr = 231.25 ml. The volume of oxygen gas at 800 torr pressure will be 231.25 ml.
A 125.0 mL sample of nitrogen at 790 torr was compressed to a volume of 75.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
Using Boyle's Law (P1V1 = P2V2), we can find the final pressure with the initial pressure (P1 = 790 torr), initial volume (V1 = 125.0 mL), and final volume (V2 = 75.0 mL). Plugging in the values: (790 torr)(125.0 mL) = P2(75.0 mL). Solving for P2 gives a pressure of 1327 torr for the trapped nitrogen.
What is the density of oxygen gas at 77 degrees C and 700 Torr?
The density of oxygen gas at 77°C and 700 Torr pressure is approximately 1.429 g/L.
A 200 ml sample of hydrogen is collected over water at 745.5 torr and 290K If the vapor pressure of water at 290k is 14.5 torr What is the volume of dry hydrogen at STP The answer is 181m?
To find the volume of dry hydrogen at STP, we need to correct for the presence of water vapor. First, calculate the pressure of dry hydrogen by subtracting the vapor pressure of water from the total pressure: 745.5 torr - 14.5 torr = 731 torr. Then, apply the ideal gas law to solve for the volume of dry hydrogen at STP: V = (200 ml * 731 torr * 273 K) / (290 K * 760 torr) ≈ 181 ml.
A 100.0 mL sample of nitrogen at 810 torr was compressed to a volume of 72.0 mL in a syringe What was the pressure of trapped nitrogen in torr?
1100
How to convert percent oxygen into pO2 Torr?
transver it though diffrent containers
A 100 ml sample of nitrogen at 810 torr was compressed to a volume of 72 mL in a syringe What was the pressure of trapped nitrogen in torr?
To find the final pressure of the nitrogen, we can use Boyle's Law which states that the pressure and volume of a gas are inversely proportional when temperature is constant. Therefore, 100 mL * 810 torr = 72 mL * final pressure. Solving for final pressure, we get: final pressure = (100 mL * 810 torr) / 72 mL = 1125 torr. So, the pressure of the trapped nitrogen in the syringe is 1125 torr.
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
If the temperature is constant, the volume of the gas will decrease with decreasing pressure according to Boyle's Law, which states that pressure and volume are inversely proportional at constant temperature. This means that as pressure decreases, volume will decrease proportionally.
The gases in a mixture have the following partial pressures at the same volume and temperature 1013000 Pa nitrogen 700 mm argon 1.20 ATM of helium 790 torr oxygen and 0.50 ATM of carbon dioxide?
Carbon dioxide Argon Oxygen Helium Nitrogen
