The combustion of toluene has a ΔErxn of −3.91 × 103kJ/mol. When 1.70 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 23.36 ∘C to 36.67 ∘C. Find the heat capacity of the bomb calorimeter to three sig-figs.
q = m*c_s*deltaT
The Attempt at a Solution
ΔErxn of −3.91 × 103kJ/mol
so ΔErxn of .0184mol toluene = 0.0184* −3.91 × 103kJ/mol = 71.944kJ/mol
c_s = q/(m*deltaT) = -71.944kJ/mol / (1.7g*13.31deg)
(i just want to make sure I calculated this correctly before I submit it (mastering physics) thanks