What is the volume in liters of 15.0 Kg of CO2 at STP.?
154637
first you convert to grams = 15000 grams\nthen 44 grams per mole\n22.4 liters per mole\n\nanswer= 15.2 liters CO2\n\n=D\n\nhope that helped
585074
Generally its between 1.5 and 2.5 litres
309325
Since m*C*dT=Q;\n\nHeat capacity=135000 J/(5100 g*(31.5K - 18K))= 1.96 J/gK\n\n(K for Kelvin)
878297
Assuming 1 mole (28.01348 g) N2 = 22.4 liters at STP, I get (28.01348*.00220102/22.4) =  0.0027526 g if collected at STP. Correcting by 273/293 * (1.5*760-17.5)/760 (for temp., press. and water) = 0.003788 g. \nSo I basically agree with your results. What's the ans. supposed to be?
1111363
graduated cylinder or callibrated pipette are the answers to the test questions in my classroom.  And in scientific situations, volume is measured in liters/litres- except when measured in cc's (cubic centimenters)
638965
What is "Dry N2 gas?"  My chemistry's a bit rusty, but here's what you might do:\n\nYou take your 40 liters and with the 22C and .956atm, you can determine how many moles of N2 you have.\n\nThen, you take those moles and apply it to whatever "Dry N2 gas" means.  My best guess would be STP.  Then you find the volume at the new temperature and pressure.
167746
At STP, 1 mole of any ideal gas will have a volume of 22.4 Liters.\nUsing this logic, we can deduce that at STP, and equal volumes of (what we will assume are ideal gasses) gasses will each contain the same number of moles.\nIf each flask contains the same number of moles, then they much each contain the same number of molecules.\n\nBy saying that the flasks are at STP, we are given all the information we need to solve this.  STP (Standard temperature and pressure) implies a temperature of 273 K and a pressure of 1 atm.
911209
volume is measured in liters or cubic meters
865243
C3H6 +  9/2 O2 ---> 3 CO2 + 3 H2O\nassumed oxygen is ideal gas, so\nPV=nRT\nR = 82.057 cm3.atm/gmol.K\nV = 15 l = 15000 cm3 ; T = 37 C = 310 K\nn (mol) O2 = PV/RT = 2.4*15000/82.057*310 = 1.415 gmol\nfrom balanced reaction CO2 = 3/(9/2) * 1.415 gmol = 0.943 gmol\n                                         = 0.943 * 44 = 41.507 gram
806996
the moles of O2  : 4/32 = 0.125\nthe volume occupied by O2 at STP : V = n*22.4 = 0.125 * 22.4 =2.8L
641078
I think this is how you would solve this problem. Use the equation PV=nRT, re-arrange to solve for V. \n\n(STP = standard temperature and pressure = 1 atm of pressure and 273 Kelvins)\n\nV = nRT/P = (1 mol)(0.0821 L*atm/k*mol)(273)/1 atm = 22.4 L
1076679
According to Boyle's Gas Law, the product of the pressure and volume of an ideal gas is a constant.\n\nTherefore, P1V1 = P2V2\nHere, P1 = 5 psi, V1 = 20 cubic inches, P2 = 10 psi.\n\nPutting into the equation,\n5*20 = 10*?\n\nAnswer is 10 cubic inches - B in the list of choices.
765956
A) 1\nB)2 moles of gas. ,1 mole of gas takes up 22.4 liters, so 44.8 L
596291
Assuming the volume of Ethylene and water is NOT additive and the calculation is done in STP.\n\nDensity of water = 1g/1ml therefore 2100g = 2.1L water\n\nUsing Equation: Delta T = i(Kb)m\n\n22C = [(1.86C/m)(x)]/2.1L\nSolving for x = 22.58mol Ethylene glycol\n\nSince Molar Mass of Ethylene glycol = 62.06g/mol\n\n22.58mol(62.06g/mol) = 1401.31g of Ethylene glycol Needed.\n\nConverting to correct Sig Fig: 1401.31g = 1400g Ethylene.\n\n(Technically your answer should be 1000g due to One sig fig in 20 degrees in Celcius, but you usually never want to put any answer in 1 S.F., so I would leave it with 2 S.F.  I hope this helps.)
776910
1 mole of an ideal gas occupies 22.4 liters, so multiply that by your number of moles and you would have the total volume occupied by this amount of gas at STP.
749394
divide the 15.8 g by the gfw ( molecular weight of Lithium chloride )
644831
The fast way to do this is to know that there are 22.4 liters per mole at STP for a gas.  The long answer is to use a gas law like the ideal gas law.  You should know from your class what gas law to use, but the ideal gas law is\n\nPV = nRT\n\nWhere \n  P = Pressure (1 atm at STP)\n  V = Volume (45 Liters)\n  n = number of moles\n  R = gas constant\n  T = temperature (298 deg C at STP)