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 = 300 gT1​ = 30 °C → T2​ = 60 °Cq = ?

How much heat q is needed to warm 300 g of water from 30 °C to 60 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 300 gT1 = 30 °CT2 = 60 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 150 gT1​ = 28 °C → T2​ = 75 °Cq = ?

How much heat q is needed to warm 150 g of water from 28 °C to 75 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 150 gT1 = 28 °CT2 = 75 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Aluminiumm = 150 gT = 180 °Cc = 0.897 J/(g·°C)Waterm = 400 gT = 17 °Cc = 4.18 J/(g·°C)

A 150 g block of aluminium (c = 0.897 J/(g·°C)) at 180 °C is dropped into 400 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 = 180 °Cmwater = 400 gTwater = 17 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Leadm = 50 gT = 150 °Cc = 0.129 J/(g·°C)Waterm = 150 gT = 23 °Cc = 4.18 J/(g·°C)

A 50 g block of lead (c = 0.129 J/(g·°C)) at 150 °C is dropped into 150 g of water (c = 4.18 J/(g·°C)) at 23 °C in an insulated cup. Find the final temperature Tf.

mmetal = 50 gcmetal = 0.129 J/(g·°C)Tmetal = 150 °Cmwater = 150 gTwater = 23 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
HCH4​ + 2O₂reactantsCO₂ + 2H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction CH4 + 2O₂ → CO₂ + 2H₂O(l).

ΔH°f(CH4) = −74.8 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
ΔH° = kJ
6.Hard
H2CH3​OH + 3O₂reactants2CO₂ + 4H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction 2CH3OH + 3O₂ → 2CO₂ + 4H₂O(l).

ΔH°f(CH3OH) = −238.7 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
ΔH° = kJ

Answer key

  1. 1. q = 37.62 kJ
  2. 2. q = 29.47 kJ
  3. 3. Tf = 29.14 °C
  4. 4. Tf = 24.29 °C
  5. 5. ΔH° = −890.3 kJ
  6. 6. ΔH° = −1453 kJ

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