Question

what is the theoretical enthalpy of KNO3 (s) mixed in H2O (l) ? based on the experimental and theoretical yield what is the percent error? I get a high percent... doesnt seem right...

what is the theoretical enthalpy of HCl (l) mixed in NaOH (aq) ? based on the experimental and theoretical yield what is the percent error? I get a high percent... doesnt seem right

75.15 Hao 3 0 13 10 - Part A Reaction 1: Heat of Solution KNO, 21. 7 Final Temperature 17. 7 Initial Temperature °C °C AT (from plot) -3.6°C_not from the data above) (referente P9.8) erelothermie Mass KNO: 7.00139 H,O volume: 75./_ (0.5 mL) 95.1 me, 'L=0.0751L Mass of solution (): (show all calculations) D y hoogin mass of KNO: 7.00939 s asintado o 9 = 75.1 g H₂O mass of H₂O: 82.1 AH experimental (show all calculations) amp T = (82.1 ) (4.184 )(-2 0 q reaction - 1236, 6 J x 1 x = -1,2366 kJ DH Exp = 1.2195kJ 0.0693 mol SH EXP = 17.57 kJ/mol moles KNO3 = 7.0093 g KNO3 = 0.0693 ma kroz 101.102 glamol 17.57 kJ/mol AH (theoretical): (see page 8) (show all calculations) KNO, 5) + H2O ) -KND -492.7 -285.9 -457,8 AH-mol(-452.725 /mall] -ml-492.7 57-1)+Imel(-2358 25/1] H = - 457.9 xml + 980.43 H = 320.8 kJ/mol 320.3 kJ/mol Percent Error: (show all calculations) % H L AH *100 = (sta. S-1757_ t 320.9 = 94.5% . Rev. F17 Page 11 of 15

Answer 1

In the problem when kno3 is mixed with water ,here the dissolution of kno3 occurs when positively charged k ions are attracted to partially negative charged oxygen atoms of water molecules and negatively charged nitrates ions are attarcted to partially positively charged hydrogen atoms of water molecules, so kno3 dissolves in water.

And also the theoretical value is 35.8kj/mol.

And also for the HCl +Naoh the theoretical value -13.75kcal/mole on converting it is -57.475 ki/mol.....