Question

A 1.800-g sample of solid phenol (c6h5oh(s)) was burned in a bomb calorimeter whose total heat capacity is 11.66 kj/∘c. the temperature of the calorimeter plus contents increased from 21.36∘c to 26.37∘c. part a write a balanced chemical equation for the bomb calorimeter reaction.

Answer 1

_____Balanced Chemical eqn___ C6H5OH + 7O2 --> 6C02 + 3H20 Firstly, heat of rxn will be absorbed by bobm calorimaeter, so find the qcal qcal = CΔT = (11.66 KJ/°C)(26.37°C- 21.36°C) = 58.42 KJ since the heat of rxn absorbed by calorimeter, assume: qrnx = -qcal = - 58.42 KJ _____q GRAM OF C6H5OH______ Find the number of moles you have by dividing the given grams of C6H5OH by its molar mass (1.8 g C6H5OH)(94 g/mole C6H5OH) = 0.0191 mol C6H5OH then divide qrnx by the number of moles. (-58.42 KJ)/(0.0191 mol C6H5OH) = -3058.64 KJ/mol C6H50H