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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.
What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure exerted by the carbon dioxide gas is 22.8 torr. This can be calculated using the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Given the mass of the gas, the number of moles can be calculated and used to determine the pressure.
Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22C and 100 kPa?
The ideal gas equation.PV = nRT22o C = 295.15 Kelvin(750 Torr)(X volume) = (1.5 moles O2)(62.36 L*torr/mol*K)(295.15 K)Volume = 27608.331/750= 37 Liters oxygen gas=================
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
When a sample of neon with a volume of 648 mL and a pressure of 0.985 ATM was heated from 16.0 to 63.0 C its volume became 689 mL What was its final pressure in ATM?
Using the combined gas law equation (P1V1/T1 = P2V2/T2), we can calculate the final pressure. Plugging in the given values, we get: 0.985 ATM * 648 mL / 289 K = P2 * 689 mL / 336 K. Solving for P2 gives a final pressure of approximately 1.02 ATM.
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
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.
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.
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 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 pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2 degrees C when it occupies a volume of 5.00 L?
The pressure exerted by the carbon dioxide gas is 22.8 torr. This can be calculated using the ideal gas law equation, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Given the mass of the gas, the number of moles can be calculated and used to determine the pressure.
Which equation is set up correctly to determine the volume of a 1.5 mole sample of oxygen gas at 22C and 100 kPa?
The ideal gas equation.PV = nRT22o C = 295.15 Kelvin(750 Torr)(X volume) = (1.5 moles O2)(62.36 L*torr/mol*K)(295.15 K)Volume = 27608.331/750= 37 Liters oxygen gas=================
As the pressure of a gas at 760 torr is changed to 380 torr at a constant temperature the volum of the gas will?
Boyle's law states that pressure is indirectly proportional to the volume. There fore as the pressure of a gas at 760 torr is changed to 380 torr, the volume will increase. Boyle's Law: P1 x V1 = P2 x V2 Rearranging leads to: P1 / P2 = V2 / V1 Substituting our values: 760 / 380 = V2 / V1 Thus the final volume will be twice the initial volume.
When a sample of neon with a volume of 648 mL and a pressure of 0.985 ATM was heated from 16.0 to 63.0 C its volume became 689 mL What was its final pressure in ATM?
Using the combined gas law equation (P1V1/T1 = P2V2/T2), we can calculate the final pressure. Plugging in the given values, we get: 0.985 ATM * 648 mL / 289 K = P2 * 689 mL / 336 K. Solving for P2 gives a final pressure of approximately 1.02 ATM.
One torr is equal to?
1 Torr = 0.00133322 bar 1 Torr = 133.322 Pa 1 Torr = 0.00131578584 ATM 1 Torr = 1 mmHg
