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A gas sample occupies a volume of 12.0 L at 50oC and 700 Torr. How many moles of gas are contained in the sample?
V = 12 LT = 50⁰C = 273 + 50 = 323 KP = 700 torr R = 62.363577 L.Torr / K.molPV = n RT 700×12 = n ×62.363577 ×...
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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 sample of nitrogen occupies 5.50 liters under a pressure of 900 torr at 25oC. At what temperature will it occupy 10.0 liters at the same pressure? Show Complete Solution.
V1/T1= V2/T25.5/298= 10/T20.0185T2= 10T2= 10/0.0185= 540.54K
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If 96.5 moles of an ideal gas occupies 41.5 liters at 301 K, what is the pressure of the gas?
PV = nRT P = nRT/V P = 96.5*8.31*301/41.5 = 5816,3 kPa
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an unknown gas occupies 10dm3 of space at 4 atm and 20°c. what is the amount in moles of the gas present if the gas is a real gas? take R = 0.082
PV=nRTP = 4 atm = 405 kPaT = 293,15 oKn= PV/RT = (405×10)/(8.2×293.15) = 1.68 molAnswer: 1.68 mol.
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A gas sample occupies 3.25 liters at 24.5 degrees Celsius and 1825 mm hg. Determine the temperature at which the gas will occupy 4250 ml at 1.50 atm
V1=3,25 L V2=4250 ml=4,25 L t1=24,5 C (273 +24,5)=297,5 K P2=1,5 atm =151,95 kPa P=1825 mm hg =243,25 kPa t2= ??? P1V1=nRT1 P2V2=nRT2 nR=const P1*V1/T1=P2*V2/T2 T2=P2*V2*T1/P1*V1 T2=(151,95*4,25*297,5)/243,25*3,23=242,8 t2=242,8
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A sample of N2 has 1.70 moles and occupies 3.80 l at 25.0˚C.
A) What volume will it occupy with 2.60 moles?
B) How many moles are in a sample that occupies 1.45 L?
According to the ideal gas law: pV=nRT p ndash; pressure (atm) V ndash; volume (L) n ndash; amount (moles) R ndash; universal gas constant T ndash; temperature (K) P, R,...
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A sample of a gas occupies a volume of 1100 mL at 78ºC and 0.060 atm. What would be the new volume if the temperature decreased to 44ºC and the pressure increased to 1.31 atm?
p1 = 0,06 atm = 6079,5Pa V1 = 1100ml = 0,0011m3 T1 = 780C = 351 K p2 = 1,31 atm = 132735,8Pa T2 = 440C = 317 K V2...
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A sample of carbon dioxide occupies a volume of 3.50 liters at 125 kPa pressure>
What pressure would the gas exert if the volume was decreased to 2.00 liters?
According to the combined ideal gas equation:p1V1 = p2V2where p1 - initial pressure, V1 - initial volume, p2 - final pressure, V2 - final volume.From here:p2 = p1V1 / V2...
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A sample of carbon dioxide occupies a volume of 3.50 liters at pressure 125 kPa. What pressure would the gas exert if its volume was decreased to 1.75 liters?
Boyle's Law can be expressed as P1V1 = P2V2initial pressure P1 = 125 Kpainitial volume V1 = 3.50 Lfinal pressure P2= ??final volume V2 = 1.75 LHence P2 = P1V1/V2P2 = 125 KPa...
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