Use PV =nRT ( pressure at STP is 1 atmosphere and temp. is 298.15 Kelvin )
(1 atm)(volume) = (1.50 mole)(0.08206 Latm/molK)(298.15 K)
= 36.7 Liters
Approx. 1 mol.
the ratio between HCL and CL2 is 4:2 V(Cl2)=0.98/2=0.49L
I would assume chlorine gas and standard temperature an atmospheric pressure. Using the ideal gas equation. PV = nRT (1 atm)(X volume) = (2.4 moles Cl2)(0.08206 Mol*K/L*atm)(298.15 K) Volume = 59 Liters of chlorine gas --------------------------------------------
Since you don't specify the conditions, I will use the current STP. At STP of 0oC (273.15 K for gases) and 100 kPa, the molar volume of a gas is 22.711 L/mol.4.50 mol Cl2 x 22.711 L/mol = 102 L Cl2, rounded to three significant figures.Just in case your teacher is using the older version of STP of 0oC (273.15 K for gases), and 1 atm, the molar volume of a gas would be 22.414 L/mol.4.50 mol Cl2 x 22.414 L/mol = 101 L Cl2, rounded to three significant figures.
91%
ClF3
At 22.4 liters a mole at STP, and the molar mass of Cl2 being 71, 17.32 g is about .242 moles. Multiply the moles by standard volume and you get 5.43 liters.
Some conversion required.30 pounds Cl2 (454 grams/1 pound) = 13620 grams Cl213620 grams Cl2 (1 mole Cl2/70.9 grams) = 192.1 moles Cl270o F = 21.1o C = 294.3 Kelvinuse,PV = nRT(743 mm Hg)(X Volume) = (192.1 moles Cl2)(62.36 L*torr/mol*K)(294.3 K)Volume = 3525524.47/743= 4.7 X 103 Liters of chlorine gas------------------------------------------
0.016L
Balanced equation for Sodium and Chlorine is: 2Na + Cl2 --> 2NaCl
stupid question
the ratio between HCL and CL2 is 4:2 V(Cl2)=0.98/2=0.49L
I would assume chlorine gas and standard temperature an atmospheric pressure. Using the ideal gas equation. PV = nRT (1 atm)(X volume) = (2.4 moles Cl2)(0.08206 Mol*K/L*atm)(298.15 K) Volume = 59 Liters of chlorine gas --------------------------------------------
Since you don't specify the conditions, I will use the current STP. At STP of 0oC (273.15 K for gases) and 100 kPa, the molar volume of a gas is 22.711 L/mol.4.50 mol Cl2 x 22.711 L/mol = 102 L Cl2, rounded to three significant figures.Just in case your teacher is using the older version of STP of 0oC (273.15 K for gases), and 1 atm, the molar volume of a gas would be 22.414 L/mol.4.50 mol Cl2 x 22.414 L/mol = 101 L Cl2, rounded to three significant figures.
91%
Cl2)+ 3 F2 = 2 ClF3
ClF3
Cl2 + 2NaBr => Br2 + 2NaCl One mole Cl2 reacts with 2 moles NaBr Cl2 = 71 NaBr = 102.9 Molar volume = 22.414 L/mole for ideal gas @STP 3L Cl2 = 3/22.414 = 0.1338 mole 25g NaBr = 25/102.9 = 0.2430 mole 0.1338 moles Cl2 requires 0.2676 moles NaBr for complete reaction The NaBr is the limiting reagent