Question

need help on 5 and 6

0 2.00 g of octane, C8H18 was burned in a bomb calorimeter causing the temperature to increase from 21.0°C to 35.5°C. The total heat capacity of the calorimeter was 0.05 KJP C. Calculate the heat of combustion for the reaction shown below. 2 C8H18(1) + 2502(g) → 16 CO2(g) + 18 H2O(g) 6. When 50.0 mL of 0.100 M AgNO3 was reacted with 50.0 mL of 0.100 M HCl in a . Styrofoam cup calorimeter, the temperature increased from 22.6°C to 23.4°C. Calculate AH for the following reaction assuming the density and specific heat of the solutions are 1.00 g/mL and 4.18 J/gºC respectively. AgNO3(aq) + HCl(aq) → AgCl(s) + HNO (aq)

Answer 1

Дитин = - о ДТ Given Ccal - 8.33 kJ/°C, AT = T2-7, = 35.5-21.0 = 14.5 °C Ahmn = -8.33/k] 1x = -120.785 kJ mass of octane = 2.5 g Molar mass of octant = 1288 + 1881 Co Co Hid) = 114 g/mol than mole of octane = 2.5.2 - = 0.021929 mol 114 Again g/mol CA Hann - 120.785 k] =-5508.00 kJ/mol 01021929 moke ţ octane Now given reaction 2 (SHis + 25 0₂ 16CO2 + 1SH2O 2 mole used in this seaction? (AH) riven Rxn = -5508.00(k) x 2 mol =-11016.00 kJ

mass s solution - density X Volume (m) = 1 2 1 x (50 + 50 m2 = 100 g Specific Heat ($1 = 4.18 Ilgol AT = T2-T, = 2314 - 22.6 = 0.80 q= (m) x (8) (AT) = 100 (7) * 4.18/3-J * (018) (C) q - 334.4 J AH = -q= -334,4]

to calculade per mole, An mole of AgNO3 = Melarity X Volume in litre = 0.100 x 50 x 103 = 0.005 mole released per mole AH = - 334.4 J Heat Mole 0.oos Mole - - 66880 /mole - - 66.88 kJ/mole In given reaction only I mole & Ag Noz used so AH for given reaction = (-66.88 KI J x 4 mole) = - 66.88 k] Mole