Answer:
-108.7 kJ / mol H₂SO₄
Explanation:
The reaction of NaOH with H₂SO₄ is:
2 NaOH + H₂SO₄ → 2H₂O + 2NaSO₄
<em>2 Moles of NaOH reacts per mole of H₂SO₄</em>
This reaction, as all acid-base reactions, produce heat. Moles of NaOH and H₂SO₄ reacting are:
0.0500L × (1.00mol NaOH / L) = 0.0500 moles NaOH
0.0500L × (0.50mol H₂O₄ / L) = 0.0250 moles H₂SO₄
Coffer cup calorimeter formula is:
Q = -C×m×ΔT
<em>Where Q is heat, C is specific heat of solution (4.18J/g°C), m is mass of solution (50g NaOH + 50g H₂SO₄ = 100g of solution -Assuming densities of 1.00g/mL), and ΔT is temperature change (31.9°C-25.4°C = 6.5°C).</em>
Replacing:
Q = -4.18J/g°C × 100g × 6.5°C
Q = -2717J
This is the heat produced in neutralization reaction when 0.0250 moles H₂SO₄ react. Now, heat per mole of H₂SO₄ is:
-2717J / 0.0250 moles H₂SO₄
= -108680 J / mol H₂SO₄ ≡ -<em>108.7 kJ / mol H₂SO₄</em>
