1.How much heat is evolved when 27.0 g of glucose is burned according to this equation?
C6H12O6 + 6O2 → 6CO2 + 6H2O; Δ H comb. = -2808 kJ/mol
2.How much heat is required to melt 200 grams of ice?
The heat of fusion is 333 J/g.
3. Calculate the amount of heat absorbed by 10.0 grams of ice at -15.0°C as it is converted to liquid water at 50.0°C. The specific heat of H2O(s) = 2.09 J/(g°C). The specific heat of H2O(l) = 4.18 J/(g°C). The heat of fusion is 333 J/g.
4.From the following data,
H2 (g) + Cl2 (g) → 2HCl(g) ΔHv = -185 kJ
2H2 (g) + O2 (g) → 2H2O(g) ΔH = -483.7 kJ
calculate ΔH for the following reaction.
4HCl(g) + O2 (g) → 2Cl2 (g) + 2H2O(g)
5.Given the following information,
SO3 (g) + H2O(l) → H2SO4 (l) ΔH = -133 kJ
Pb(s) + PbO2 (s) + 2H2SO4(l) → 2PbSO4(s) + 2H2O(l) ΔH = -509 kJ
calculate the ΔH for the reaction below.
Pb(s) + PbO2 (s) + 2SO3 (g) → 2PbSO4 (s)
1 . Amount released when 27.0 g is burned is 421.2 KJ 2. Heat is required... View the full answer