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Q: The vapor pressure of 10 mL of ethanol at 20 degrees C is 5.85 kPa. What is the vapor pressure of 20 mL of ethanol at the same temperature
A: 11.7 kPa
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User: The vapor pressure of 10 mL of ethanol at 20 degrees C is 5.85 kPa. What is the vapor pressure of 20 mL of ethanol at the same temperature

Weegy: 11.7 kPa
cr7|Points 112|

User: A gas has a volume of 590 mL at a temperature of –55.0 C. What volume will the gas occupy at 30.0 C?

User: A gas occupies a volume of 140 mL at 35.0 degrees C and 97 kPa. What is the volume of the gas at STP?

Weegy: Use the Ideal Gas Law: V = (nRT)/P Remember to use atm. for pressure, K for temp. and L for volume. [ First, find how many moles of the gas there were (solve for n) Then, using that amount of the gas, find the volume it would occupy if it were at STP Oh, and STP = T = 273K, P = 1 atm. and R (ideal gas constant) = 0.0821 Here is the work: 140ml = 0.140 L; 35C = 308 K; 97 kPa = 0.9576 atm Ideal gas equation rearranged to solve for moles: n = (PV)/(RT) (0.9576*0.14)/(0.0821*308) = .005301738 moles V = nRT/P (but now use STP) V = (.005301738*0.0821*273)/1atm V = 0.1188 L If you think about it, this makes sense because the volume in fact would be lower since you are lowering the temperature and increasing the pressure (two things that decrease the volume) ]
Controler|Points 3928|

User: What is the mole fraction of KCl in a 0.20 molal solution of KCl? (molar mass of KCl = 75 g; molar mass of water = 18 g)

Weegy: "0.20 mole solution of KCl" are you sure it's "0.20 mole"? - THe question would be meaningless for this case Or is it "0.20 MOLARS"? - additional facts is needed (e.g. [ density of solution, density of KCl) Or is it "0.20 MOLALS"? - the sol'n would be the following: 0.20 molal KCl sol'n = 0.20 mol KCl / 1 kg H2O for every kg of water in the solution, there are: 0.20 mol KCl 1 kg H2O = 1000 g H2O = 1000/18 mol H2O = 55.56 mol H2O mol fraction of KCl = (mol KCl) / (mol KCl + mol H2O) mol fraction of KCl = (0.20) / (0.20 + 55.56) mol fraction of KCl = 0.00359 (just adjust the # of sig fig) ]
tarungehlot|Points 50|

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Asked 2/27/2013 8:55:54 PM
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