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a cylinder contains 1.475 x 10^24 argon atoms. how many moles of argon are there in the cylinder
1 mole of argon = 6.02 × 1023= 1.475 × 1024/6.02 × 1023= 2.4502 moles of argon
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A flask contains 2.00 moles of nitrogen and 2.00 moles of helium. How many grams of argon must be pumped into the flask in order to make the partial pressure of argon twice that of helium?
You can use the following law for solving this question: PfVf = P1V1 + P2V2 + P3V3 hellip; etc Pf is final pressure of the mixture Vf is Final volume...
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A flask contains 3.00 moles of nitrogen and 3.00 moles of neon. How many grams of argon must be pumped into the flask in order to make the partial pressure of argon twice that of neon?
The partial pressure of individual gas in the gas mixture can be expressed the following way: Pi = Ptotal *xi, Where Pi – is the partial pressure of individual gas...
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A vessel of 2×10⁻³m³ volume contains 0.036 kg of Argon at 300K. Calculate its pressure using ideal gas equation. ( Atomic mass of Ar = 39.9u).
V= 2x10-3m3 = 2dm3m= 0.036Kg = 36gT= 300KR= 0.0821L.atm/k.molnumber of moles, n= mass/Molar mass = 36/39.9= 0.9molPV= nRTP= nRT/Vp= 0.9x0.0821x300/2P= 11.08atm
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Given that the molar mass of argon gas is39.95 g/mil,if 2.00 mil of argon can effuse from an opening in a vessel in 3.626 seconds and 1.00 mols of gas X can effuse in 1.000 seconds.identify gas X
79.9= 3.626? = 179.9× 1/3.626= 22.0422.04/211.02Nitrogen gas
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An unknown liquid was found to have a density of 69.22lb/ft3. The density of ethylene glycol (the liquid used in antifreeze)is 1.1088 g/mL. Is the unknown liquid ethylene glycol?
69.22lb/ft3=1.1088 g/mL.Therefore the unknown liquid is ethylene glycol.
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How is Vapor Pressure of a liquid related to the intermolecular forces within that liquid?
How does vapor pressure change with Temperature? When does a liquid boil?
Vapor pressure is a property of a liquid based on the strength of its inter-molecular forces. A liquid with weak inter-molecular forces evaporates more easily and has a high vapor...
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112 mL of NO2(g) at STP was liquefied, the density of the liquid being 1.15 g mL
Calculate the volume of liquid and the number of molecules in the liquid NO2
One mole of an ideal gas will occupy a volume of 22.4 liters at STP (Standard Temperature and Pressure, 0°C and one atmosphere pressure).Proportion:1 mole – 22400 mln moles –...
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The reduction of titanium (IV) chloride to titanium cannot be carried out in air. The air has to be replaced with argon gas. Explain why air needs to be replaced with argon gas for this reaction.
QUESTION # 136434The reduction of titanium (IV) chloride to titanium cannot be carried out in air. The air has to be replaced with argon gas. Explain why air needs to...
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The liquid 1-iodobutane has a density of 1.62 g/mL at 20.0 °C. If a 143 gram sample of this compound is needed, what volume of the liquid at 20.0 °C must be provided? volume=...............ml
Volume = Mass / Density = 143g / 1.62g/mL = 88.27mL
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