16,8 L of Xe gas at STP is equivalent to 0,754 moles.
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. To find the number of moles in 168 liters of CO2, you can divide 168 by 22.4, which gives approximately 7.5 moles. Since the molar mass of CO2 is about 44 grams per mole, you can multiply 7.5 moles by 44 grams/mole to find that 168 liters of CO2 contains approximately 330 grams.
0.25 moles
8,4 liters of nitrous oxide at STP contain 2,65 moles.
The answer is 0,2675 moles.
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At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters. To find the number of moles in 168 liters of CO2, you can divide 168 by 22.4, which gives approximately 7.5 moles. Since the molar mass of CO2 is about 44 grams per mole, you can multiply 7.5 moles by 44 grams/mole to find that 168 liters of CO2 contains approximately 330 grams.
210.3 moles of H2 are contained in one gallon of H2O
PV = nRT ⟹ n = PV/RT = 1 * 18.65 / (0.082 * 273.15) = 0.8321 moles.
1 mole of any gas occupies 22.4 L at standard temperature and pressure (STP). Therefore, 8.08 L of O2 at STP would contain 8.08/22.4 = 0.36 moles of O2.
0.25 moles
8,4 liters of nitrous oxide at STP contain 2,65 moles.
At STP, 1 mole of any gas occupies 22.4 L. Therefore, in a 5L sample of argon at STP, there would be 5/22.4 moles of argon, which is approximately 0.223 moles.
The answer is 2,68 moles.
The answer is 0,2675 moles.
See the Related Question "How do you solve Ideal Gas Law problems?" to the left for the answer.
Assuming ideal behaviour, 1 mole of any gas occupies 22.4L at STP. So, moles of 10L = 10/22.4 moles = 0.4464 moles
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