[T33]

The problem I am having issues with is about the amount of heat given off in burning cyclohexane along with the amount of grams needed to burn. Here is the exact wording.

A hospital autoclave made of steel has a mass of 32 kg. It is filled with 352 grams of water. The temperature of both is 23.7 C. You want to heat them both to 100 C. To do that you will use the heat given off when you burn cyclohexane. If all the heat given off in burning the cyclohexane is used to heat the autoclave filled with water, how many grams of cyclohexane will you need to burn to achieve that ?

The specific heat capacity Cs of H2O = 4.18 J/ g C and of Steel = 0.45 J/ g C. The enthalpy of combustion of C6H12 is -4010 kJ/mole. Your answer should be in grams of C6H12 needed.

I started by calculating the heat needed ( using the q=mcΔT)
I made sure to convert the mass of steel to grams so it then became 32,000g
and my final answers of q were:
q steel: 341,280 J
q h20: 34,871 J

Although I am very unsure whether I have gone about this problem the proper way.

[XeLa.]

Your initial going-about the problem is a good start, however, I would make sure that you understand what the ΔT in your equation signifies.

Okay, once you've recognised that, from where you're at, what do you think you'll next need to consider? You're told to find how many grams of cyclohexane will need to be burned to give off this amount of heat. What data are you given about cyclohexane?

XeLa