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 = 500 gq = 47 kJΔT = ?

47 kJ of heat is added to 500 g of water (c = 4.18 J/(g·°C)). Find the temperature rise ΔT.

q = 47 kJm = 500 gc = 4.18 J/(g·°C)
ΔT = °C
2.Easy
waterm = 750 gT1​ = 20 °C → T2​ = 40 °Cq = ?

How much heat q is needed to warm 750 g of water from 20 °C to 40 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 750 gT1 = 20 °CT2 = 40 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Aluminiumm = 150 gT = 100 °Cc = 0.897 J/(g·°C)Waterm = 150 gT = 17 °Cc = 4.18 J/(g·°C)

A 150 g block of aluminium (c = 0.897 J/(g·°C)) at 100 °C is dropped into 150 g of water (c = 4.18 J/(g·°C)) at 17 °C in an insulated cup. Find the final temperature Tf.

mmetal = 150 gcmetal = 0.897 J/(g·°C)Tmetal = 100 °Cmwater = 150 gTwater = 17 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Aluminiumm = 75 gT = 100 °Cc = 0.897 J/(g·°C)Waterm = 100 gT = 19 °Cc = 4.18 J/(g·°C)

A 75 g block of aluminium (c = 0.897 J/(g·°C)) at 100 °C is dropped into 100 g of water (c = 4.18 J/(g·°C)) at 19 °C in an insulated cup. Find the final temperature Tf.

mmetal = 75 gcmetal = 0.897 J/(g·°C)Tmetal = 100 °Cmwater = 100 gTwater = 19 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
H2C4​H10​ + 13O₂reactants8CO₂ + 10H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction 2C4H10 + 13O₂ → 8CO₂ + 10H₂O(l).

ΔH°f(C4H10) = −125.6 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
ΔH° = kJ
6.Hard
HC6​H12​O6​ + 6O₂reactants6CO₂ + 6H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction C6H12O6 + 6O₂ → 6CO₂ + 6H₂O(l).

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

Answer key

  1. 1. ΔT = 22.49 °C
  2. 2. q = 62.7 kJ
  3. 3. Tf = 31.66 °C
  4. 4. Tf = 30.23 °C
  5. 5. ΔH° = −5755 kJ
  6. 6. ΔH° = −2802 kJ

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