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.

New worksheetPractise online with hints

For teachers: free to print, copy and use in class. Every new worksheet has new values and its own answer key. A link to ExamProblems on your course page is appreciated.

Name: ____________________   Date: ____________

1.Easy
waterm = 750 gq = 16 kJΔT = ?

16 kJ of heat is added to 750 g of water (c = 4.18 J/(g·°C)). Find the temperature rise ΔT.

q = 16 kJm = 750 gc = 4.18 J/(g·°C)
ΔT = °C
2.Easy
waterm = 250 gT1​ = 25 °C → T2​ = 50 °Cq = ?

How much heat q is needed to warm 250 g of water from 25 °C to 50 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 250 gT1 = 25 °CT2 = 50 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Aluminiumm = 75 gT = 120 °Cc = 0.897 J/(g·°C)Waterm = 200 gT = 22 °Cc = 4.18 J/(g·°C)

A 75 g block of aluminium (c = 0.897 J/(g·°C)) at 120 °C is dropped into 200 g of water (c = 4.18 J/(g·°C)) at 22 °C in an insulated cup. Find the final temperature Tf.

mmetal = 75 gcmetal = 0.897 J/(g·°C)Tmetal = 120 °Cmwater = 200 gTwater = 22 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Aluminiumm = 250 gT = 90 °Cc = 0.897 J/(g·°C)Waterm = 400 gT = 24 °Cc = 4.18 J/(g·°C)

A 250 g block of aluminium (c = 0.897 J/(g·°C)) at 90 °C is dropped into 400 g of water (c = 4.18 J/(g·°C)) at 24 °C in an insulated cup. Find the final temperature Tf.

mmetal = 250 gcmetal = 0.897 J/(g·°C)Tmetal = 90 °Cmwater = 400 gTwater = 24 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
H25 g CH3​OH2CH3​OH + 3O₂reactants2CO₂ + 4H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 25 g of CH3OH (M = 32.04 g/mol) burns completely: 2CH3OH + 3O₂ → 2CO₂ + 4H₂O(l). Give q as a positive number.

ΔH°f(CH3OH) = −238.7 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
q = kJ
6.Hard
H20 g C3​H8​C3​H8​ + 5O₂reactants3CO₂ + 4H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 20 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

Answer key

  1. 1. ΔT = 5.104 °C
  2. 2. q = 26.13 kJ
  3. 3. Tf = 29.3 °C
  4. 4. Tf = 31.81 °C
  5. 5. q = 566.8 kJ
  6. 6. q = 1007 kJ

Full step-by-step solutions: practise this topic on examproblems.com.