A12.8 g sample of ethanol (c2h5oh) is burned in a bomb calorimeter with a heat capacity of 5.65 kj/°c. using the information below, determine the final temperature of the calorimeter if the initial temperature is 25.0°c. the molar mass of ethanol is 46.07 g/mol.
delta h rxn = -1235
c2h5oh + 3o2 -> 2co2 +3h2o

The final temperature of the calorimeter is 85.71 degree C.

Heat of the reaction is -1235 kJ/mol

Heat discharged at the time of reaction is 1235 kJ/mol

The moles of ethanol are calculated by using the formula mass of ethanol / molar mass of ethanol

= 12.8 g / 46 g/mol = 0.278 moles

Thus, the no. of moles of ethanol is 0.278 moles

The heat released when ethanol is combusted is:

0.278 moles × 1235 kJ/mol = 343 kJ

The final temperature is determined as,

343 kJ = (heat capacity) (temperature difference)

343 kJ = 5.65 (T - 25)

T-25 = 343 / 5.65

T-25 = 60.71

T = 85.71 degree C

Thus, the final temperature is 85.71 degree C.

dynamic equilibrium is the answer.

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