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What will be the volume of 1g of helium at ntp in liters?
At NTP (standard temperature and pressure), which is 0 degrees Celsius and 1 atm pressure, the volume occupied by 1 gram of helium would be approximately 22.4 liters. This value is based on the ideal gas law and the molar mass of helium.
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.
A 6.00L gas tank contained a mixture of helium and oxygen at a pressure of 20.1 ATM. If the mixture was 75 helium what were the partial pressures of oxygen and helium?
To find the partial pressures of helium and oxygen in the gas tank, we can use Dalton's Law of Partial Pressures. Given that the mixture is 75% helium, the partial pressure of helium (P_He) is 75% of the total pressure: P_He = 0.75 × 20.1 ATM = 15.075 ATM. The remaining 25% is oxygen, so the partial pressure of oxygen (P_O2) is 25% of the total pressure: P_O2 = 0.25 × 20.1 ATM = 5.025 ATM.
A balloon has a volume of 6.3 liters Calculate the mass of helium that it would take to fill the balloon?
To calculate the mass of helium, you would need to know the density of helium (0.1785 g/L at 0°C and 1 atm). You can use the formula: mass = density x volume. In this case, mass = 0.1785 g/L x 6.3 L = 1.125 g.
What volume will 4.0 mol of helium gas occupy at 300 K and 2.0 ATM?
You can use the ideal gas law to find the volume:PV = nRTV = nRT/P (use R=0.08206 L*atm/mol*K)= (4.0 mol)*(0.08206 L*atm/mol*K)*(300K)/(2.0 atm)V = 49.24 L
What will be the volume of 1g of helium at ntp in liters?
At NTP (standard temperature and pressure), which is 0 degrees Celsius and 1 atm pressure, the volume occupied by 1 gram of helium would be approximately 22.4 liters. This value is based on the ideal gas law and the molar mass of helium.
What is the volume of oxygen occupied by 2 moles at 1.3 ATM pressure at 300 k?
38 L
What is the volume of oxygen occupied by 2 mole at 1.3 ATM pressure and 300 K?
38 L
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 volume of oxygen occupied by 2 moles at 1.3 ATM pressure and 300 K Use PV nRT.?
38 L
How many milliliters would be occupied by 0.234 g of NH3 at 30 oC and a pressure of 0.847 atm?
The volume is 402 mL.
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
What is volume occupied by a mole of an ideal gas if the pressure is 626mmHg and the temperature is 25.0C?
The volume occupied by a mole of an ideal gas can be calculated using the ideal gas law equation: PV = nRT. Convert the pressure to atm (1 atm = 760 mmHg), and the temperature to Kelvin (25.0°C = 298 K). Then substitute the values into the equation and solve for volume (V).
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.
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
What volume is occupied by 1.00 kg of helium at 5.00 degrees celsius at a pressure of 735 torr?
Well, we might as well convert all of this mess. ( we could work in Torr, but why when we are mass converting )1.00 kg He (1000 grams/1 kg) = 1000 grams He (1 mole He/4.003 grams) = 250 moles He5.00o Celsius = 278.15 Kelvin735 Torr = (1 atm/760 Torr = 0.967 atmospheres=========================================Now,PV = nRT(0.967 atm)(Volume) = (250 moles He)(0.08206 L*atm/mol*K)(278.15 K)0.967V = 5706.247Volume = 5.90 X 103 Liters-----------------------------------
A balloon has a volume of 6.3 liters Calculate the mass of helium that it would take to fill the balloon?
To calculate the mass of helium, you would need to know the density of helium (0.1785 g/L at 0°C and 1 atm). You can use the formula: mass = density x volume. In this case, mass = 0.1785 g/L x 6.3 L = 1.125 g.
