First find out how many moles of gas are collected under the given conditions using the Ideal Gas Law.See the Related Questions link to the left for how to do that. Then use that number of moles and determine the volume of that much gas at STP, also using the Ideal Gas Law question to the left.
The molar volume of any ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Converting 39.6 dm3 to liters gives 39.6 L. To find the mass of argon gas, we calculate the number of moles using the ideal gas equation (PV = nRT) and then multiply by the molar mass of argon.
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
xenon is a gas at STP
Volume of a gas at STP (standard temperature and pressure) refers to the volume that a gas occupies when measured at a temperature of 0 degrees Celsius and a pressure of 1 atmosphere. This volume is typically given in liters or cubic meters.
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First find out how many moles of gas are collected under the given conditions using the Ideal Gas Law.See the Related Questions link to the left for how to do that. Then use that number of moles and determine the volume of that much gas at STP, also using the Ideal Gas Law question to the left.
STP stands for Standard Temperature and Pressure. At STP, the pressure of natural gas is 1 atm, and 1 mole of gas takes up 22.4 liters.
Fluorine is a gas at standard temperature and pressure (STP), which is defined as 0 degrees Celsius and 1 atmosphere of pressure.
Argon is a gas at STP. It becomes a liquid below -186oC and solid below -190oC at StP
At standard temperature and pressure (STP), the gas that occupies the highest volume is hydrogen.
1 mole of gas at STP (standard temperature and pressure) occupies 22.4 liters of volume. This is known as the molar volume of a gas at STP. Additionally, the gas has a pressure of 1 atmosphere and a temperature of 273 K at STP.
While STP is at 25oC (298 K) and 1 ATM, the ideal gas law (P1.V1 / T1 = P2.V2 / T2) states the following solution: [T2/T1]*[P1/P2]*V1 = V2[(273+25.0) K / (273+20.0) K] * [3.00 atm / 1.00 atm] * 720.0 mL =[298.0 / 293.0] * [3.00] * 720.0 = 2197 mL
No, fluorine is a diatomic gas at standard temperature and pressure (STP), meaning it exists as F2 molecules, not as single F atoms.
The volume of a mole of any gas at Standard Temperature and Pressure (STP) is approximately 22.4 liters. This is known as the molar volume of a gas at STP and is a standard value used in gas calculations.
The state depends on the temperature and pressure. At STP, radon is a gas.
To find the volume of the oxygen gas at STP (standard temperature and pressure), you can use the combined gas law. First, convert 25ºC to Kelvin by adding 273, giving you 298 K. Then use the equation (P1V1)/T1 = (P2V2)/T2, where P1 = 458 mmHg, V1 = 828 mL, T1 = 298 K, P2 = 760 mmHg (STP pressure), T2 = 273 K (STP temperature). Solve for V2 to find the volume of the oxygen gas at STP.