Question

Enter your answer in the provided box. A quantity of 2.00 x 102 mL of 0.477 M HCl is mixed with 2.00 x 102mL of 0.239 M Ba(OH), in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the HCl and Ba(OH)2 solutions is the same at 20.45°C. For the process below, the heat of neutralization is -56.2 kJ/mol. What is the final temperature of the mixed solutions? H(aq) + OH(aq) H20(1).

Answer 1

Answers Here, we have to find the final temperature of the mined Solution : given, reaction is W traqltott (aq) ) Hzole Malarity of Hcd, M = 0.477M 122.00* 62me llaume of the " X 1000 M= Ime M *u n . La 1000 0.477 X 200 = 1030 5 n n = 0.477 I n=0.045h holes Therefore, Hol Contains one Htion = 0.0954 moles . No.of moles of Htion ,دلع Molarity of Balot)2 = 0.239 M (colume of Balottle = 2:00*10²m2 =200m nouot mores of Balottle = houdens-10005 0239 X 200 0.0668

one Balo), contains a moles of otions Therefore, соназ мо(е» 4 и он ), Conta, a 2 + он18 -0.0956 moles Now, Ht tot H20,8 SH 3-56.2 kJ/mol. For Imole of Nutralization the heat released = -5612 kilnot for = -56.2. 0.0956 moles of nutralization = -5.37 kg There fore, q = -5.37 kJ li 9 = -537 ¥1037 This heat is absorbed by the water 9 = mSAT lblume of water = Volume of Cacid + Base ) - Hook 10²ml density = 1 gelme mass of wated = volume of water x density = 4:00*102 L x 19 mass of water = 400*10?g

specific heat of water = 14 1865/9°c ST = Tfinal - Tinitial where, q=msst 5.34*103 = (hoog) (4.186.5/9c) (Tf -204542 Ps - 20145 = - Thoog) (14.186 5/9°c) 5:37 X 103 If - 20.45 = 3.21c Tf = 13.21 +20:45) c Tf = 23.66°C Therefore, The final temperature of solution = 23.66°C) or