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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 mixture of Helium and Neon gases is collected over water at 28 degree Celsius and 745 mm Hg. If the partial pressure of Helium is 368 mm Hg, what is the partial pressure of Neon? Please explain.
The vapor pressure at 28 Co is of 28.3 mm Hg. Based on the Dalton’s law regarding partial pressure of gas mixture the total pressure is defined as follows: P...
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If a balloon is filled with He, Ne, and Ar gases at a total pressure of 2.0atm, what is the partial pressure of argon if the partial pressures of helium and neon are both 0.25atm each?
According to Dalton's law of partial pressure:Ptotal = P1 + P2 + P3 ...where Ptotal - total pressure, Pn - partial pressureHere:Ptotal = PHe + PNe + PArAs a result,...
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In the decomposition of phosphoric acid, H3PO4(s), pyrophosphoric acid and water form. How many moles of phosphoric acid are needed to produce 8.34mol of pyrophosphoric acid?
2H3PO4(s) = H2O + H4P2O7According to the equation, 1 mole of pyrophosphoric acid requires 1 mole of phosphoric acid. Therefore, 8.34 moles of pyrophosphoric acid require 8.34 x 2 =...
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A 2.0 dm³ container contains 0.15 mol of N₂ gas and 0.20 mol of O₂ gas under a total pressure of 100 kNm⁻². Calculate the partial pressure of O₂ gas in the mixture.
Solution:Calculate the mole fraction (x) of O2 gas in the mixture:x(O2) = number moles of O2 / total number moles of gasTotal number moles of gas = Moles of...
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<ol><li>Calculate the volume of the original sample needed if you would use a 50 mL volumetric flask, a 100 mL volumetric flask, and a 250 mL volumetric flask to prepare a dilution of 1:25.</li></ol>
Ratio 1:25 means that there have to be 1+25 = 26 equal parts.1) The volume of the original sample needed if we would use a 50 mL volumetric flask is...
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what is the average mass of neon if 90.48% of neon is neon-20, 0.27% of neon is neon-21, and 9.25% of neon has 12 neutrons?
m= 0.9048 x 20 + 0.27 x 21 + 0.0925 x 22=20.1877 g.
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If some neon gas at 121,000 Pa were allowed to expand from 37 mL to 60 mL without changing the temperature, what pressure would the neon gas exert under these new conditions?
pV=nRT. n=0.121 x 37 / 8.314 x 273. = 0,00197248826.p= nRT/V=0,00197248826 x 8.314 x 273 / 60 = 0,0746166667 kpa.74.616 pa.
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A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The
total pressure is 1.50 atm. Calculate the partial pressures of the gases.
p(CH4) = 0.55 atmp(C2H6) = 0.44 atmp(C3H8)= 0.51 atm
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