Cracking the Code: Calorimetry Worksheet 2 Answers (Chemsheets)

Let’s be real—calorimetry can feel like a juggling act. One minute you’re calculating temperature changes (ΔT), the next you’re wrestling with specific heat capacity (c), and just when you think you’re done, someone throws in q = mcΔT for the third time just to be sure.

Why is experimental ( \Delta H ) less than theoretical?
Heat loss to surroundings, incomplete combustion, non-standard conditions.

Balanced Thermochemical Equations
Where required, answers include fully balanced equations with correct state symbols and ( \Delta H ) values.

Fully Worked Answers
Every question from Chemsheets Calorimetry Worksheet 2 is answered with clear, line-by-line working. See exactly how to apply ( q = mc\Delta T ) and convert between joules, kilojoules, and kJ/mol.

If your answers aren't matching the mark scheme, check these three common errors: Unit Conversion: Did you convert from Joules to kiloJoules ( /1000/ 1000 ) before calculating ΔHcap delta cap H ? Most worksheet answers are in The Sign (+/-): If the temperature went up, your final ΔHcap delta cap H value must have a minus sign.

Have you tried the worksheet and hit a wall? Drop the question number in the comments—I’ll walk you through it.

(Mass): Usually the mass of water or the solution being heated (e.g., 200g of water or the combined volume of two solutions assuming a density of (Specific Heat Capacity): Almost always taken as for water. ΔTcap delta cap T

  1. Neutralisation reactions (e.g., HCl + NaOH)
  2. Combustion of alcohols or fuels
  3. Dissolving salts in water
  4. Finding specific heat capacity of a metal