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 = 100 gT1​ = 25 °C → T2​ = 95 °Cq = ?

How much heat q is needed to warm 100 g of water from 25 °C to 95 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 100 gT1 = 25 °CT2 = 95 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 150 gT1​ = 29 °C → T2​ = 40 °Cq = ?

How much heat q is needed to warm 150 g of water from 29 °C to 40 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 150 gT1 = 29 °CT2 = 40 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Leadm = 250 gT = 180 °Cc = 0.129 J/(g·°C)Waterm = 400 gT = 16 °Cc = 4.18 J/(g·°C)

A 250 g block of lead (c = 0.129 J/(g·°C)) at 180 °C is dropped into 400 g of water (c = 4.18 J/(g·°C)) at 16 °C in an insulated cup. Find the final temperature Tf.

mmetal = 250 gcmetal = 0.129 J/(g·°C)Tmetal = 180 °Cmwater = 400 gTwater = 16 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Leadm = 100 gT = 200 °Cc = 0.129 J/(g·°C)Waterm = 250 gT = 17 °Cc = 4.18 J/(g·°C)

A 100 g block of lead (c = 0.129 J/(g·°C)) at 200 °C is dropped into 250 g of water (c = 4.18 J/(g·°C)) at 17 °C in an insulated cup. Find the final temperature Tf.

mmetal = 100 gcmetal = 0.129 J/(g·°C)Tmetal = 200 °Cmwater = 250 gTwater = 17 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
HC2​H5​OH + 3O₂reactants2CO₂ + 3H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction C2H5OH + 3O₂ → 2CO₂ + 3H₂O(l).

ΔH°f(C2H5OH) = −277.7 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
ΔH° = kJ
6.Hard
HC3​H8​ + 5O₂reactants3CO₂ + 4H₂O(l)productsΔH° = ?

Use the standard enthalpies of formation to find ΔH° for the reaction C3H8 + 5O₂ → 3CO₂ + 4H₂O(l).

ΔH°f(C3H8) = −103.8 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 = 29.26 kJ
  2. 2. q = 6.897 kJ
  3. 3. Tf = 19.1 °C
  4. 4. Tf = 19.23 °C
  5. 5. ΔH° = −1367 kJ
  6. 6. ΔH° = −2220 kJ

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