Two calorimeters each contain 1.4L of water and have a temperature of 26°C
In the first calorimeter, you burn a sample of candle wax and determine that 108.2kJ of energy is released. In the second calorimeter, you have to burn 5.4g of candle wax to raise the temperature of the water from 26°C to 53°C.
What is the mass of the candle wax used in the first calorimeter?
First, I did some conversions:
1.4L = 1400mL = 1400g (due to something about the equal density of water (1g/mL)
108.2kJ = 108200J
-And the specific heat capacity of water is 4.184 J/g°C
ΔT = Tf - Ti = 53°C - 26°C = 27°C
So I started off with (for the second calorimeter):
Q = mcΔT
Q = (1400g)(4.184J/g°C)(27°C)
Q = 160000J of thermal energy absorbed by the water, and released by the burning of the candle wax
Then...
-160000J -> 5.4g
-108200J -> x
x = 3.69g of candle wax was used in the first calorimeter
Is this correct?