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What is the total pressure of a mixture containing two gases if the partial pressure of one gas is 70 torr and the partial pressure of the other gas is 30 torr?
P1 = 70 torr , P2 = 30 torrPTotal = P1 + P2 PTotal = 70 torr + 30 torr = 100 torr
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At 25°C, the vapor pressure of benzene, C6H6, is 95 torr, snd toluene, C7H8, is 28 torr. Find the total pressure of the solution containing 30% C6H6 and 70% C7H8.
30% of 95torr = 28.570% of 28 torr= 19.6Total pressure = 28.5+19.6= 48.1 torr
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150 ml of gas are enclosed in the cylinder under a pressure of 760 torr. What would be the volume be at pressure of 1520 torr?
.p(1) *V(1)= p(2) *V(2) From which V(2)= p(1) *V(1)/p(2)=150*760/1520=75 ml
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A gas sample occupies 5.63 liters at 776 torr. Find the volume of the same gas if the pressure is changed to 827 torr.
Volume of the gas=5.278litres
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A 2.00 L sample of gas originally at 25 °C and pressure of 400 torr is allowed to expand
to a volume of 5.00 L.
If the final pressure of gas is 585 torr, what is the final temperature in K?
p*V = n*R*Tn and R are constant so p*V/T = constantThen (2.00 L)*(400 torr)/(25+273.15 K) = (5.00 L)*(585 torr)/TT = (5.00 L)*(585 torr)*(25+273.15 K)/(2.00 L)/(400 torr) = 1090 K
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A mixture of 90.0 grams of CH4 and 10.0 grams of argon has a pressure of 250 torr under conditions of constant temperature and volume. The partial pressure of CH4 in torr is:
Molar mass of CH4 = 16.04 g/molMolar mass of argon = 39.9g/molFrom the given masses we can calculate number of moles followed by mole fraction of each gas.Number of moles...
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A mixture of four gases exerts a total pressure of 860mmHg. Gas A and B each exert 220mmHg. Gas C exerts 110mmHg. What pressure is exerted by gas D?
For this task we use the Dalton’s law which says that total pressure of mixture of gases equals to the sum of partial pressures of individual gases: Ptotal=PA+PB+PC+PD Therefore PD...
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A sample of oxygen occupies a volume of 250. mL at a pressure of 704. torr. What volume will the gas occupy at a pressure of 800. torr if temerature is held constant
P1×V1= P2×V2 V2 = P1×V1/P2 V2 = 704×250/800 = 220. ml Answer: 220. ml.
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What is the partial pressure of sulfur dioxide gas in torr in a sealed vessel that has a total pressure of 520 torr and partial pressures of 0.35 atm for nitrogen?
P_gen=P(〖SO〗_2 )+P(N_2) P(〖SO〗_2 )= P_gen-P(N_2) 1 atm = 760 torr P(N_2 )=(760 torr×0.35 atm)/(1 atm)=266 torr P(〖SO〗_2 )= 520-266=254 (torr) Answer: 254 torr.
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A 1.00-L gas sample at 100.°C and 600. torr contains 49.0% helium and 51.0% xenon by mass. What are the partial pressures of the individual gases?
100 g of gas = 49 g of He and 51 g Xe n(He) = 49 / 4 = 12.25 mol n(Xe) = 51 / 131.29 = 0.388 mol n(He)...
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