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​ = 19 °C → T2​ = 45 °Cq = ?

How much heat q is needed to warm 1000 g of water from 19 °C to 45 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 1000 gT1 = 19 °CT2 = 45 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 400 gT1​ = 27 °C → T2​ = 70 °Cq = ?

How much heat q is needed to warm 400 g of water from 27 °C to 70 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 400 gT1 = 27 °CT2 = 70 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Leadm = 100 gT = 170 °Cc = 0.129 J/(g·°C)Waterm = 150 gT = 16 °Cc = 4.18 J/(g·°C)

A 100 g block of lead (c = 0.129 J/(g·°C)) at 170 °C is dropped into 150 g of water (c = 4.18 J/(g·°C)) at 16 °C in an insulated cup. Find the final temperature Tf.

mmetal = 100 gcmetal = 0.129 J/(g·°C)Tmetal = 170 °Cmwater = 150 gTwater = 16 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Leadm = 200 gT = 150 °Cc = 0.129 J/(g·°C)Waterm = 250 gT = 21 °Cc = 4.18 J/(g·°C)

A 200 g block of lead (c = 0.129 J/(g·°C)) at 150 °C is dropped into 250 g of water (c = 4.18 J/(g·°C)) at 21 °C in an insulated cup. Find the final temperature Tf.

mmetal = 200 gcmetal = 0.129 J/(g·°C)Tmetal = 150 °Cmwater = 250 gTwater = 21 °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
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

Answer key

  1. 1. q = 108.7 kJ
  2. 2. q = 71.9 kJ
  3. 3. Tf = 19.1 °C
  4. 4. Tf = 24.11 °C
  5. 5. ΔH° = −890.3 kJ
  6. 6. ΔH° = −5755 kJ

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