How much heat is absorbed by the calorimeter if the temperature change is 12 C and the calorimeter constant (Heat Capacity) is 3.3 J/K?
q = 3.3 J/K * 12
How much heat is absorbed by the calorimeter if the temperature change is 8 C and the calorimeter constant (Heat Capacity) is 3.3 J/K
To calculate the amount of heat absorbed by the calorimeter, you can use the formula:
Q = C * ΔT
Where:
Q is the heat absorbed or released (in joules)
C is the calorimeter constant or heat capacity (in joules per degree Celsius or joules per Kelvin)
ΔT is the change in temperature (in degrees Celsius or Kelvin)
In this case, you are given:
ΔT = 12 C
C = 3.3 J/K
To calculate Q, you need to convert the temperature difference to Kelvin since the heat capacity should be in joules per Kelvin.
ΔT(K) = ΔT(C) + 273.15
So, ΔT(K) = 12 + 273.15 = 285.15 K
Now, you can substitute the values into the formula:
Q = C * ΔT(K)
= 3.3 J/K * 285.15 K
= 940.395 J
Therefore, the calorimeter absorbs approximately 940.395 joules of heat.