A sample of Freon-12 (CF2Cl2) occupies 25.5 L at 298 K and 153.3 kPa. Find its volume at STP.?
926278
i did away with all that crap and just put in 134a, sorry!
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
780066
V = nRT/P\nV = (25g/44g/mol)(0.08206Latm/molK)(298K)/1atm\nV = 138.9 L
178984
To do this, you need to employ the ideal of PV=nRT.  You have the values for P, V, R, and T.  Plug those into the equation to find moles.  Then, plug the number of moles in with STP values, and solve for Volume at STP.  That's it.
759551
V1/T1 = V2/T2\n\nFirst convert temperature to Kelvin. 198+ 273 = 471\n\nNext plug into equation\n\n4.81 L / 471 K = 2.49 L / T2\nT2 = 243.8\nthen put it back into C 243.8 - 273 = -29.2 C
766934
Assume it is an ideal gas and use PV = nRT\n\nP is in atm 1 atm = 760 torr\n    225 torr / 760 torr = 0.296 atm\nV is in L so 5.7 L\nR is 0.0821 atm*L/mol*K\nT is in K so C + 273 = K\n     27 + 273 = 300 K\n\n(0.296)(5.7) = (0.0821)(300)n\nn = 0.0685 mols
750705
212 F, 100 C,     373 K
482555
AgBr-------->Ag+ + Br-\n(a) Ksp=[Ag][Br] solubility=s=[Ag]=[Br]=Ksp^0.5\ns=(6*10^-7)^0.5\n(b) [Br]=0.01 (because all of kBr was dissuciated)\ns=Ksp/[Br]=(6*10^-7)/0.01 mol/lit
385149
density of H2 at STP = d= PM /RT\n\nd= density  =X\n\nP= pressure  =1atm\n\nM= molar mass = 2.016g of H2\n\nR= gas constant = .0821\n\nT=temperature  = 273K\n\n\nX= .0899g/L\n\n\n 1.6g H2 corrected to STP: \n\n\n1.6gH2(.0899g/L / 2.016gH2)= .0713g/L
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.
924197
PCO2 = 35-45\nPO2 = 75-100
945060
Ksp = [Pb2+][F-]^2 = 2.69E-8\n\nThe number of fluorine moles will be double the number of lead moles from the PbF2, but there are also 0.470 mol/L of F- ions from the NaF.  So, you can simplify the Ksp equation to Ksp = x * (2x + 0.1175)^2, where x is the number of moles of PbF2 that will disolve in the solution.\n\nSolve x:\nKsp = x * (4x^2 + 0.470x + 0.0138) = 4x^3 + .470x^2 + 0.0138 x\n2.69 E-8 = 4x^3 + .470x^2 + 0.0138 x\nx = 1.949 E-6 mol/L\nFor your 250 mL solution, that is 1.949E-6 / 4 = 4.872 E-5 mol\nWith a molecular weight of 245.2 g/mol, that is 4.872 E-5 * 245.2 = 1.195 E-4 g, or 1.20 E-4 g.\n\nGood luck!
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.
585380
Assuming the temperature is 298K (25oC) The equation is P1V1/T1 = P2V2/T2\n\nWith temperature in Kelvin and Pressure in dm-3\n\nSo P2=1*0.50*333/(298*0.66)\n=0.847Pa
889156
The answer is BrF3.\n\nand the balance equation is \n\nBr2  +  3F2  --->  2BrF3\n\nhow? get the moles of each using this formula:\nn = PV/RT\n\nyou'll get:\nmol Br2 = 0.041mol\nmol F2 = 0.123 mol\nmol pdt = 0.082 mol\n\nbase from this, you'll found that ratio of Br:F is 1:3. Hence, the product is BrF3. you'll also found that ratio of Br2:F2:pdt is 1:3:2 which also agrees with our balance equation above.
902790
First, you find the pressure of Cl2.  Then you use PV=nRT to find the moles of Cl2.  Then you convert moles of Cl2 into the mass of Cl2\n\nThe total pressure is the sum of the partial pressures.\n\nTotal pressure = Pressure of CH4 + Pressure of Cl2\n\nPressure of Cl2 = Total pressure - Pressure CH4\n\nPressure of Cl2 = 0.445 - 0.145 = 0.300 atm\n\nNow just use the formula PV=nRT to find the moles of Cl2:\n\nPV = nRT\n\nn = PV/RT\n\nn = (0.300)(.403)/(0.0821)(301)\n\nn = 4.89 x 10^(-3) moles of Cl2\n\nMass of Cl2 = moles of Cl2 * molar mass of Cl2\n\nMass of Cl2 = (4.89 x 10^-3) * (2*35.45)\n\n*** Mass of Cl2 = 0.35 g
422875
U have not mentioned the gas gravity to determone deviation factor to have an exact answer...generally..taking z=1\npsia ( absolute value) will also be used \nPsc*Vsc/Tsc=PV/T\n\nso: Vsc/V=PTsc/PscT=53.1/T \n\nThis is the simplest correct answer.... make is easier but worse that the process is isothermal so\n\nVsc/V=102 --> 1cu ft at TVD= 102 SCF\n\nThe most exact solution can be provided if u want..with taking temperatire and deviation,composition in account