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 gT1​ = 11 °C → T2​ = 85 °Cq = ?

How much heat q is needed to warm 500 g of water from 11 °C to 85 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 500 gT1 = 11 °CT2 = 85 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 300 gq = 26 kJΔT = ?

26 kJ of heat is added to 300 g of water (c = 4.18 J/(g·°C)). Find the temperature rise ΔT.

q = 26 kJm = 300 gc = 4.18 J/(g·°C)
ΔT = °C
3.Medium
Tf​ = ?Leadm = 50 gT = 180 °Cc = 0.129 J/(g·°C)Waterm = 200 gT = 18 °Cc = 4.18 J/(g·°C)

A 50 g block of lead (c = 0.129 J/(g·°C)) at 180 °C is dropped into 200 g of water (c = 4.18 J/(g·°C)) at 18 °C in an insulated cup. Find the final temperature Tf.

mmetal = 50 gcmetal = 0.129 J/(g·°C)Tmetal = 180 °Cmwater = 200 gTwater = 18 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Zincm = 50 gT = 110 °Cc = 0.388 J/(g·°C)Waterm = 250 gT = 25 °Cc = 4.18 J/(g·°C)

A 50 g block of zinc (c = 0.388 J/(g·°C)) at 110 °C is dropped into 250 g of water (c = 4.18 J/(g·°C)) at 25 °C in an insulated cup. Find the final temperature Tf.

mmetal = 50 gcmetal = 0.388 J/(g·°C)Tmetal = 110 °Cmwater = 250 gTwater = 25 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
H50 g C3​H8​C3​H8​ + 5O₂reactants3CO₂ + 4H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 50 g of C3H8 (M = 44.1 g/mol) burns completely: C3H8 + 5O₂ → 3CO₂ + 4H₂O(l). Give q as a positive number.

ΔH°f(C3H8) = −103.8 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
q = 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 = 154.7 kJ
  2. 2. ΔT = 20.73 °C
  3. 3. Tf = 19.24 °C
  4. 4. Tf = 26.55 °C
  5. 5. q = 2517 kJ
  6. 6. ΔH° = −2220 kJ

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