Enthalpy Practice Worksheet

  1. Compound A is burned in a bomb calorimeter that contains 2.50 liters of water. If the combustion of 0.175 moles of this compound causes the temperature of the water to rise 45.00 C, what is the molar heat of combustion of compound A? The heat capacity of water is 4.18 J / g·K.
  2. Compound B is burned in a bomb calorimeter that contains 1.50 liters of water. When I burned 50.0 grams of compound B in the calorimeter, the temperature rise of the water in the calorimeter was 35.00C. If the heat of combustion of compound B is 2,150 kJ/mol, what is the molar mass of compound B?
  3. The molar heat of combustion of compound C is 1,250 kJ/mol. If I were to burn 0.115 moles of this compound in a bomb calorimeter with a reservoir that holds 2.50 L of water, what would the expected temperature increase be?
  4. When 1 mole of methane (CH4) is burned at constant pressure, 890 kJ of energy is released as heat. Calculate ∆H for a process in which a 5.8 g sample of methane is burned under constant pressure.
  5. When 1.00g of sodium hydroxide is dissolved in 100.0 g of water in an insulated container the temperature rises from 20.00°C to 22.66°C. Calculate the enthalpy change for the solution. State any assumptions made. NOTE: Dissolving reactions due not have limiting reagents.
  6. When 100.0 ml of 1.00 moldm-3NaOH is added to 100.0 ml of 1.00 moldm-3HCl in an insulated container the temperature rises from 21.0°C to 34.6°C. NaOH(aq) + HCl (aq) NaCl(aq) + H2O(l) Calculate the enthalpy change for the neutralization reaction. State any assumptions made.
  7. Aluminum has a specific heat of 0.902 Jg-1 K-1. How much heat is lost when a piece of aluminum with a mass of 23.984 g cools from a temperature of 415.0° C to a temperature of 22.0° C?
  8. The temperature of a sample of water increases by 69.5°C when 24,500 J are applied. The specific heat of liquid water is 4.18 Jg-1 K-1. What is the mass of the sample of water?
  9. Calculate how much energy in kJ is needed to warm 250.0 ml water from 25.0 °C to 95.0 °C in order to make a cup of coffee. (250 ml = 250 g)
  10. Determine the specific heat capacity of methanol if 1.80 x102 J of heat is added to 70 g of liquid methanol and its temperature increases from 18.5°C to 30.5° C.
  11. In cooking “Crepe Suzette”, a delicious type of French pancake one tablespoon (2.50g) of brandy (containing ethanol) is poured over the pancakes and then it is ignited.
  12. The molar mass of the ethanol is 46.08 gmol-1. Calculate the number of moles of ethanol, C2H5OH in the tablespoon.
  13. The enthalpy change for the reaction is –1350 kJmol-1 . Calculate the heat released when the brandy on the Crepe Suzette burns
  14. 10.0 g of NaOH is added to 100.0 g of water at 23.2°C in a glass beaker. The solution is stirred and the maximum temperature of 44.6°C is reached.
  15. Calculate the heat produced by the reaction. (Assume the specific heat capacity of the solution is 4.20 Jg-1°C-1). Is the reaction exothermic or endothermic?
  16. Calculate the enthalpy change for dissolving the solid NaOH in water in kJmol-1.
  17. Write an equation for the dissolving process.
  18. The value given in the literature under similar conditions is -42.7 kJmol-1. Suggest a reason why the calculated value of the enthalpy change of the solution is different from the literature value and propose an improvement in the procedure to obtain a more accurate result.
  19. 50.0 cm3 of 1.00 mol dm-3copper sulfate solution is added to the calorimeter and its temperature measured every 25 s. Excess zinc powder is added after 100 s and the temperature starts to rise until a maximum after which it falls in an approximately linear fashion.Calculate the molar enthalpy change from the data in the graph below.