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)

heat released = q = Ccal x (delta T) and I would work in J again everywhere.

Then q/gram = q/1.283 = x
Convert to J/mol by x*molar mass and that needs to be conert to kJ/mol because of the directions in the problem.

So

q/1.283 = 3841(130.32)

I know you have to divide by the molar mass which I found to be 132.169 but Im not sure which number I divide it by.

No, when you have q/1.283 you have q/gram. Multiply by molar mass for q/mol, then convert to kJ/mol.

Well, well, well! Time to unleash my combustion comedy routine!

To calculate the molar enthalpy of combustion (ΔHcomb), we need to use the equation:

ΔHcomb = q / n

Where q is the heat released by the combustion and n is the number of moles of cinnamaldehyde.

Now, let's calculate q, shall we?

q = Ccalorimeter * ΔT

Where Ccalorimeter is the heat capacity of the calorimeter and ΔT is the change in temperature.

Substituting the given values, we get:

q = 3.841 kJ/C * 130.32 C

Now, let's convert the mass of cinnamaldehyde to moles, using its molar mass.

Molar mass of C9H8O = 9 * atomic mass of C + 8 * atomic mass of H + atomic mass of O

Mass of C9H8O = 1.283 g

n = Mass / Molar mass

Finally, we put it all together to find ΔHcomb!

ΔHcomb = q / n

Now, don't get burned by this equation! Give it a try and let me know if you need more help!

To calculate the molar enthalpy of combustion (ΔHcomb) of cinnamaldehyde, we can use the equation:

ΔHcomb = q / n

where:
ΔHcomb = molar enthalpy of combustion (kJ/mol)
q = heat absorbed by the calorimeter (kJ)
n = number of moles of cinnamaldehyde burned

First, we need to find the heat absorbed by the calorimeter (q). We can use the equation:

q = Ccalorimeter * ΔT

where:
q = heat absorbed by the calorimeter (kJ)
Ccalorimeter = heat capacity of the calorimeter (kJ/°C)
ΔT = change in temperature (°C)

Now, let's calculate q:

q = 3.841 kJ/°C * 130.32 °C
q = 499.65 kJ

Next, we need to determine the number of moles of cinnamaldehyde burned. We can use the molar mass of cinnamaldehyde to find the number of moles:

molar mass of C9H8O = (12.01 g/mol * 9) + (1.01 g/mol * 8) + (16.00 g/mol * 1)
molar mass of C9H8O = 104.07 g/mol

Now, let's calculate the number of moles:

n = mass / molar mass
n = 1.283 g / 104.07 g/mol
n = 0.01234 mol

Finally, we can calculate the molar enthalpy of combustion ΔHcomb:

ΔHcomb = q / n
ΔHcomb = 499.65 kJ / 0.01234 mol
ΔHcomb ≈ 40,509 kJ/mol

Therefore, the molar enthalpy of combustion (ΔHcomb) of cinnamaldehyde is approximately 40,509 kJ/mol.