gas constant R = 0.08206 L.atm / mol.K or 8.314 m3.Pa / mol.K 0 K...

gas constant R = 0.08206 L.atm / mol.K or 8.314 m3.Pa / mol.K 0 Kelvin = -273.15 OC
1) The volume of a gas at 124 OC and 1.00atm is 8.12 L. Calculate the temperature ( OC ) required to change the volume to 0.00934 m3 at constant pressure.
2) A sample of helium gas has a volume of 234 mL at 25.0 OC and 342 kPa. Calculate the temperature ( OC ) of this gas sample when occupying a volume of 540mL at 444kPa
3) Calculate the pressure ( kPa ) exerted by 73.5 g carbon dioxide gas ( 44.01 g / mol ) at 322 OC in a 65.0 liter vessel
4) Calculate the number of molecules in 5.00x10-24 m3 of oxygen gas at 94.0 OC and 154 kPa pressure.
5) Calculate the molar mass ( g ) of a gas, 3.23g of which occupies a volume of 321mL at 53OC and 0.430 atm pressure.
6) Calculate the volume ( L ) of chlorine gas produced from 299 g sodium chloride ( 58.44 g / mol ) at 142.2 OC and 1.34 atm pressure               
2 NaCl ( l )   -> 2 Na ( l ) + Cl2 ( g )
7) Calculate the density ( g / L) of nitrogen gas ( 28.01 g / mol ) at 122 OC and 1.39 atm pressure.
8) Determine the quantity ( mol ) of oxygen required for the combustion of 5.52 kg octane to carbon dioxide and water.Molar mass g : octane C8H18 114.32,    CO2 44.01      O2 32.00
9) What volume ( L ) of gaseous phosphine PH3 (125.0 OC and 7.34 atm ) will be formed by the reaction of 19.0 g of calcium phosphide ( Ca3P2, 182.2 g / mol ) with excess water. Ca3P2 ( s ) + 6 H2O   ->   3 Ca(OH)2 ( s ) + 2 PH3 ( g )   
10) Calculate the atomic weight of a metal M, 0.239 g which produces 0.00455 mol hydrogen gas from excess hydrochloric acid solution.
2 M ( s ) + 2HCl ( aq ) -> 2 MCl ( aq ) + H2 ( g ) atomic weight hydrogen 1.008 g / mol
CHEMICAL EQUILIBRIUM AND GAS BEHAVIOUR
11) Calculate the concentration ( mol / L ) of nitrous oxide, NO, formed at equilibrium in a mixture initially prepared containing 7.32 M O2, 9.32 M N2               
N2 ( g ) + O2 ( g )   <->   2 NO ( g )         KC = 2.00 x 10-4
12) Calculate the concentration ( mol / L) of chlorine, Cl2, formed at equilibrium in a mixture initially prepared containing 2.00 mol / L phosphorous pentachloride, PCl5                     
PCl5 ( g )   <-> PCl3 ( g ) + Cl2 ( g )       KC = 8.00
13) Calculate the total equilibrium pressure ( atm ) produced when 2.885 mol formamide, HCONH2, is initially added to a 5.00 L flask at 127 OC.      
HCONH2 ( g )   <-> NH3 ( g ) + CO ( g )   KC = 8.75 at 127 OC      
14) 3.88 mol of A and 4.11 mol of B are placed in a 0.640 L container. Calculate the equilibrium constant, KC, given that 1.63 mol of C was present at equilibrium :               
A ( g ) + B ( g )   <-> C ( g ) +3 D ( g )
15) A total pressure of 13.1 atm was recorded when solid ammonium carbamate was placed in a flask at 23 K to attain equilibrium. Calculate the pressure equilibrium constant, Kp                     
NH4CONH2 ( s ) <-> 2 NH3 ( g ) + CO ( g )      
16) Calculate the concentration equilibrium constant, KC, given the pressure equilibrium constant, KP = 1324, for the equilibrium at 86.0 K
NH4CONH2 ( s ) <-> 2 NH3 ( g ) + CO ( g)
17) Calculate the mass of iodine, I2, present at equilibrium after 16.128 g hydrogen and 3048 g iodine are initially inserted into a 8.00 L container at 448 OC.      
H2 ( g ) + I2 ( g ) <-> 2 HI ( g )                              
Atomic weight H 1.008 g, I 127 g Kc = 5.00 at 448 OC
18) Calculate KP for the equilibrium shown below given that a total pressure of 5.1 atm was created when 61.0 % of an initial NOBr concentration dissociated to form the equilibrium 2 NOBr ( g )   <->   2 NO ( g ) + Br2 ( g )