The thermite reaction demonstrated can be represented with this chemical equation: Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(s)
Use the following thermodynamic data to calculate ΔHrxn for this reaction. Fe2O3(s) ΔHf = –824 kJ/mol Al2O3(s) ΔHf = –1673 kJ/mol
Find the heat released for 31.0 g of Fe.
Find the final temperature (Tf) for adding that much heat to that much Fe. Useful formulas and data: q = mC(Tf – Ti) Ti = 25°C C = 0.45 J/g°C
How much heat is required to bring 31.0 g Fe to 1530°C, the melting point of Fe?
How much heat is left over after raising the temperature of the Fe to its melting point?
Is the left over heat enough to melt all 31.0 g of Fe if it takes 14.9 kJ/mol to melt it? Fe(s) → Fe(l) ΔH = +14.9 kJ/mol
Why is it safe to store pre-mixed thermite reaction mixture even though the reaction is, once started, one that cannot be stopped?