WORKSHEET#14 (Midterm 3 Review) Name: ____________________________ Date: ___________________ 1. The partial pressures of H 2 and Cl 2 in a 7.00 L container at 275 °C were measured and found to be 380. torr each. How many grams of HCl will be produced given the reaction below has a yield of 85.0% and that the reaction temperature was held constant at 275 °C? (Answer: 4.82 g) H 2 + Cl 2 → HCl 2. How many grams of NH3 will be produced from a reaction between H2 and NO is the partial pressures of H2 and NO were 536 torr and 602 torr, respectively, and a temperature of 150. ℃? Assume the reaction volume is 25.0 L and the reaction yield is 100.0%. (Answer: 3.46 g) H 2 + NO → NH 3 + H 2 O Page 1 of 3 Answer Key 275°C + 273 = 548 K 380 torn = 0.500 atm 760 2 For Hz : PV = n RT For Ck : PV = n RT - n = PVIRT - n = PVIRT = ( 0.5 atm ) ( 7.00 L ) / ( 0.0821 ) ( 548k ) = ( 0.5 atm ) ( 7.00 L ) / ( 0.0821 ) ( 548K ) n = 0.0778 mot n = 0.0778 mot 0.0778 mot Hz x I mm ! , Fft = 0.156 mol Uz x I mm ! , Haft = 0.156 mol HCl No limiting reactant 0.156 mol HCl x 36.46 of = 5.69 g HCl 1 mol HCl ( 5.69 g HCl ) ( 0.85 ) = 4.83g 5Hz t 2 NO → 2MHz t 2h20 2¥ ) 150°C t 273 = 423 IT For Hz : - 536t = 0.705 atm For NO : bojfgtorr = 0.792 atm 760 - n = PV / RT n = PVIRT = ( O . 705 atm ) (25.04/10.0821) ( 423 K ) = ( 0.792 atm ) (25.04/10.0821) ( 423 K ) n = 0.508 mot Hz n = 0.570 mot NO 0.508 mol Hz x 25mm ! ,Ntf3z=NHO . 570 mot NO x 22 Mmo ! , NNH } = 0.570 mol NHS limiting readout 0.203 not NHS x 17.04 g 1- not Nitz = 3.46g NHZ percent yield : 1.00 × 3.46g NH z = 3.46 of NHS