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 = 200 gT1​ = 11 °C → T2​ = 80 °Cq = ?

How much heat q is needed to warm 200 g of water from 11 °C to 80 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 200 gT1 = 11 °CT2 = 80 °Cc = 4.18 J/(g·°C)
q = kJ
2.Easy
waterm = 400 gT1​ = 13 °C → T2​ = 90 °Cq = ?

How much heat q is needed to warm 400 g of water from 13 °C to 90 °C? The specific heat of water is 4.18 J/(g·°C). Give the answer in kJ.

m = 400 gT1 = 13 °CT2 = 90 °Cc = 4.18 J/(g·°C)
q = kJ
3.Medium
Tf​ = ?Zincm = 150 gT = 180 °Cc = 0.388 J/(g·°C)Waterm = 100 gT = 24 °Cc = 4.18 J/(g·°C)

A 150 g block of zinc (c = 0.388 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 = 150 gcmetal = 0.388 J/(g·°C)Tmetal = 180 °Cmwater = 100 gTwater = 24 °Ccwater = 4.18 J/(g·°C)
Tf = °C
4.Medium
Tf​ = ?Zincm = 150 gT = 190 °Cc = 0.388 J/(g·°C)Waterm = 400 gT = 16 °Cc = 4.18 J/(g·°C)

A 150 g block of zinc (c = 0.388 J/(g·°C)) at 190 °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 = 150 gcmetal = 0.388 J/(g·°C)Tmetal = 190 °Cmwater = 400 gTwater = 16 °Ccwater = 4.18 J/(g·°C)
Tf = °C
5.Hard
H100 g C3​H8​C3​H8​ + 5O₂reactants3CO₂ + 4H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 100 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
H25 g C4​H10​2C4​H10​ + 13O₂reactants8CO₂ + 10H₂O(l)productsq = ?

Use the standard enthalpies of formation to find the heat q released when 25 g of C4H10 (M = 58.12 g/mol) burns completely: 2C4H10 + 13O₂ → 8CO₂ + 10H₂O(l). Give q as a positive number.

ΔH°f(C4H10) = −125.6 kJ/molΔH°f(CO₂) = −393.5 kJ/molΔH°f(H₂O, l) = −285.8 kJ/molΔH°f(O₂) = 0
q = kJ

Answer key

  1. 1. q = 57.68 kJ
  2. 2. q = 128.7 kJ
  3. 3. Tf = 43.07 °C
  4. 4. Tf = 21.85 °C
  5. 5. q = 5034 kJ
  6. 6. q = 1238 kJ

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