Calorimetry & enthalpy worksheet with answers

Free printable Calorimetry & enthalpy worksheet: 6 problems from easy to exam level, with an answer key. Print it or save it as a PDF.

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1.Easy
waterm = 200 gq = 11 kJΔT = ?

11 kJ of heat is added to 200 g of water (c = 4.18 J/(g·°C)). Find the temperature rise ΔT.

q = 11 kJm = 200 gc = 4.18 J/(g·°C)
ΔT = °C
2.Easy
waterm = 1000 gq = 9 kJΔT = ?

9 kJ of heat is added to 1000 g of water (c = 4.18 J/(g·°C)). Find the temperature rise ΔT.

q = 9 kJm = 1000 gc = 4.18 J/(g·°C)
ΔT = °C
3.Medium
Tf​ = ?Zincm = 50 gT = 80 °Cc = 0.388 J/(g·°C)Waterm = 150 gT = 15 °Cc = 4.18 J/(g·°C)

A 50 g block of zinc (c = 0.388 J/(g·°C)) at 80 °C is dropped into 150 g of water (c = 4.18 J/(g·°C)) at 15 °C in an insulated cup. Find the final temperature Tf.

mmetal = 50 gcmetal = 0.388 J/(g·°C)Tmetal = 80 °Cmwater = 150 gTwater = 15 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Ironm = 100 gT = 110 °Cc = 0.449 J/(g·°C)Waterm = 250 gT = 21 °Cc = 4.18 J/(g·°C)

A 100 g block of iron (c = 0.449 J/(g·°C)) at 110 °C is dropped into 250 g of water (c = 4.18 J/(g·°C)) at 21 °C in an insulated cup. Find the final temperature Tf.

mmetal = 100 gcmetal = 0.449 J/(g·°C)Tmetal = 110 °Cmwater = 250 gTwater = 21 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
H2C2​H6​ + 7O₂reactants4CO₂ + 6H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction 2C2H6 + 7O₂ → 4CO₂ + 6H₂O(l).

ΔH°f(C2H6) = −84.7 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
ΔH° = kJ
6.Hard
H10 g C6​H12​O6​C6​H12​O6​ + 6O₂reactants6CO₂ + 6H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 10 g of C6H12O6 (M = 180.16 g/mol) burns completely: C6H12O6 + 6O₂ → 6CO₂ + 6H₂O(l). Give q as a positive number.

ΔH°f(C6H12O6) = −1274 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
q = kJ

Answer key

  1. 1. ΔT = 13.16 °C
  2. 2. ΔT = 2.153 °C
  3. 3. Tf = 16.95 °C
  4. 4. Tf = 24.67 °C
  5. 5. ΔH° = −3119 kJ
  6. 6. q = 155.5 kJ

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