How much heat is absorbed by the calorimeter (qcal) if the temperature is increased 12.4 °C and the calorimeter constant (Ccal) is 3.30 J/°C?
qcal = 12.4 °C x 3.30 J/°C = 40.92 J
To find the heat absorbed by the calorimeter (qcal), you can use the formula:
qcal = Ccal × ΔT
Where:
qcal is the heat absorbed by the calorimeter
Ccal is the calorimeter constant
ΔT is the change in temperature
Given that the change in temperature is 12.4 °C and the calorimeter constant is 3.30 J/°C, we can substitute these values into the formula:
qcal = 3.30 J/°C × 12.4 °C
Calculating this expression will give us the amount of heat absorbed by the calorimeter.
To find the amount of heat absorbed by the calorimeter, you can use the formula:
qcal = Ccal * ΔT
where:
qcal is the heat absorbed by the calorimeter,
Ccal is the calorimeter constant,
ΔT is the change in temperature.
In this case, the ΔT is given as 12.4 °C and the Ccal is given as 3.30 J/°C.
Now, you can substitute the given values into the formula and calculate the heat absorbed by the calorimeter:
qcal = 3.30 J/°C * 12.4 °C
qcal = 40.92 J
Therefore, the heat absorbed by the calorimeter is 40.92 J.