Question

1. A solid substance has a mass of 250.00g. It is cooled by 25.00°C and loses 4.937kJ of heat. What is the specific heat capacity of the substance in ? [APP 2 marks] 2. The combustion of hydrogen sulfide, H2S can be represented by the following balanced equation: 2H2S(g) + 302(g) → 2802(g) + 2H200) Show how the following equations can be combined using Hess's Law and determine the enthalpy of combustion of hydrogen sulfide. [APP 3 marks] Ss) + O2(g) → SO2(g) H2(g) + S8)→ H2S() H2O → H2(g) + 1202(9) AH = -296.8kJ AH2 = -20.6 kJ AH3 = +285.8kJ 3. A chemist wants to determine the enthalpy change for the following reaction: C3H120) + 802(g) → 5CO2(g) + 6H2O(g) When the chemist burns 0.530g of pentane, it increased the temperature of 250mL of water from 21.0°C to 38.2°C. a) Calculate the enthalpy of this reaction, in units of kJ/mol C3H12. [APP 4 marks] b) Write a thermometric equation to represent the reaction. [APP 1 mark] c) Draw the enthalpy diagram for the reaction above. [APP 1 mark] 4. The complete combustion of 1.00mol of acetone, C3H60, releases 1790kJ: C3H00) + 402(g) → 3CO2(g) + 3H201) AH°comb = -1790kJ Calculate the enthalpy of formation of acetone. [T/I 3 marks]

Answer 1

qemCOT q = heat loses 4.937 X 1037 m= mas 2500g ca specific heat AT = Change in temperature a 25€ ca v MAT 4.937 X10% ] 250g x 25°C ca (0.789 J/g c Answer post other question seperately This is violation of HomeworkLib guidlines,