Monday
March 30, 2015

Homework Help: chem

Posted by greg on Monday, October 15, 2012 at 3:10pm.

The complete combustion of 1.283g of cinnamaldeyde (C9H8O, one of the compounds in cinnamon) in a bomb calorimeter (Ccalorimeter=3.841 kJ/C) produced an increase in temperature of 130.32 C. Calculate the molar enthalpy of combustion of cinnamaldehydy (delta H comb) (in kilojoules per mole on cinnamaldehyde)

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - The complete combustion of 1.283g of cinnamaldeyde (C9H8O, one of ...
Chemistry - The complete combustion of 1.283g of cinnamaldeyde (C9H8O, one of ...
Chemistry - The combustion of benzoic acid releases 26.38kJ/g and is often used ...
Chemistry - When 0.3212g of glucose was burned in bomb calorimeter of ...
Chemistry - The molar enthalpy of combustion of glucose is -2803 kJ. A mass of 1...
Chemistry - The molar enthalpy of combustion of glucose is -2803 kJ. A mass of 1...
Chemistry - The molar enthalpy of combustion of glucose is -2803 kJ. A mass of 1...
Chemistry - The temperature rises from 25.00 C to 29.00 C in a bomb ...
Chem - The following substances undergo complete combustion in a bomb ...
Chemistry - 2. When a 1.000 g sample of the rocket fuel hydrazine, N2H4, is ...

Members