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 = 1000 gT1​ = 15 °C → T2​ = 45 °Cq = ?

How much heat q is needed to warm 1000 g of water from 15 °C to 45 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 1000 gT1 = 15 °CT2 = 45 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 100 gT1​ = 18 °C → T2​ = 65 °Cq = ?

How much heat q is needed to warm 100 g of water from 18 °C to 65 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 100 gT1 = 18 °CT2 = 65 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Leadm = 250 gT = 180 °Cc = 0.129 J/(g·°C)Waterm = 100 gT = 24 °Cc = 4.18 J/(g·°C)

A 250 g block of lead (c = 0.129 J/(g·°C)) at 180 °C is dropped into 100 g of water (c = 4.18 J/(g·°C)) at 24 °C in an insulated cup. Find the final temperature Tf.

mmetal = 250 gcmetal = 0.129 J/(g·°C)Tmetal = 180 °Cmwater = 100 gTwater = 24 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Copperm = 150 gT = 190 °Cc = 0.385 J/(g·°C)Waterm = 400 gT = 25 °Cc = 4.18 J/(g·°C)

A 150 g block of copper (c = 0.385 J/(g·°C)) at 190 °C is dropped into 400 g of water (c = 4.18 J/(g·°C)) at 25 °C in an insulated cup. Find the final temperature Tf.

mmetal = 150 gcmetal = 0.385 J/(g·°C)Tmetal = 190 °Cmwater = 400 gTwater = 25 °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 = 125.4 kJ
  2. 2. q = 19.65 kJ
  3. 3. Tf = 35.17 °C
  4. 4. Tf = 30.51 °C
  5. 5. ΔH° = −890.3 kJ
  6. 6. ΔH° = −1453 kJ

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