Question

Alright I am doing a lab and I want to make sure I am doing the formula correctly since this for a lab and chemistry is something that requires you to learn everything or else you'll be lost the more you go into it, nonetheless here's my lab data from my three trials:
Trial 1 Trial 2 Trial 3
Mass of empty calorimeter (g) 18.600, 18.600, 18.600
Mass o f Mg (g) 0.15, 0.25, 0.35
Initial temperature To © 21.5, 21.5, 21.5
Final Temperature Tf © 34.5, 43.2, 51.8
Mass of calorimeter, HCl and Mg (g) 68.738, 68.829, 68.921,
I need to find the amount of heat gained right so I'm thinking I'm suppo

Answer 1

I'm supposed to use the Mass of calorimeter, HCl and Mg for each trial and multiply that by the change in the initial temperature from the final temperature like so: 13.1*68.738=
but this is the part I'm lost on which is do I multiply it again by 4.18 J in the end or do I only have to multiply the first two? Any help would be greatly appreciated!

Answer 2

It looks good to me.

Answer 3

So don't multiply it by 4.18 at the end or do?

Answer 4

4.18 J/\(^oC\)g is the specific heat capacity, that value is exactly the specific heat capacity of water, is that what you are supposed to use? what about the calorimeter itself?