A 12.8 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

so far I converted CHOH to moles

.2778 mol C2H5OH

then converted to KJ

.2778 mol x -1235 kJ / 1mol = 343.13 kJ

I know q = m delta temp C

So I have m = 12. 8 g
Tf= ?
Ti= 25
C = 5.65 kJ/ C

I tried to set it up this way

343kJ = 12.8 g (25- Tf)(5.65 kJ/C)

but I think I'm wrong.

Question

A 12.8 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

so far I converted CHOH to moles

.2778 mol C2H5OH

then converted to KJ

.2778 mol x -1235 kJ / 1mol = 343.13 kJ

I know q = m delta temp C

So I have m = 12. 8 g
Tf= ?
Ti= 25
C = 5.65 kJ/ C

I tried to set it up this way

343kJ = 12.8 g (25- Tf)(5.65 kJ/C)

but I think I'm wrong.