Ask Question
17 July, 11:37

A 0.1149-g sample of solid magnesium is burned in a bomb calorimeter that has a heat capacity of 1769 J/°C. The calorimeter contains exactly 321 g of water, and the temperature increases by 1.126°C. Calculate the heat given off by the burning Mg, in kJ/g and in kJ/mol.

+1
Answers (1)
  1. 17 July, 14:47
    0
    The heat given off by the burning Mg is 30.5 kJ/grams or 745.5 kJ/mol

    Explanation:

    Step 1: Data given

    Mass of magnesium sample = 0.1149 grams

    Molar mass of magnesium = 24.3 g/mol

    bomb calorimeter that has a heat capacity of 1769 J/°C

    Mass of water = 321 grams

    Temperature change = 1.126 °C

    Step 2: Calculated heat released

    Q = (1769 J/°C * 1.126 °C) + (321 grams * 4.184 J/g°C * 1.126 °C)

    Q = 3504.18 J = 3.504 kJ

    Step 3: Calculate the heat given off by the burning Mg, in kJ/g

    3.504 kJ / 0.1149 grams = 30.5 kJ/grams

    Step 4: Calculate moles of Magnesium

    Moles of magnesium = mass magnesium / Molar mass magnesium

    Moles magnesium = 0.1149 grams / 24.3 g/mol

    Moles magnesium = 0.0047 moles

    Step 5: Calculate the heat given off by the burning Mg, in kJ/mol

    3.504 kJ / 0.0047 moles = 745.5 kJ/mol

    The heat given off by the burning Mg is 30.5 kJ/grams or 745.5 kJ/mol
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A 0.1149-g sample of solid magnesium is burned in a bomb calorimeter that has a heat capacity of 1769 J/°C. The calorimeter contains ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers