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 temp
erature 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.
<span>_____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</span>
