Calorimetry defines the act of measuring different changes in state variables of a body for deriving the heat transfer related to the changes of its states. This Calorimetry is performed with a calorimeter.
Formula for Calorimetry
Q = heat evolved ( heat absorbed − heat released) in joules (J)
m = mass in kilograms (kg)
c = specific heat capacity in J/kg⋅°C (or J/kg⋅K)
∆T = temperature change in °C (or K)
Example 1: One gram of sodium hydroxide (NaOH) is dissolved in 40 mL of water at 30 °C. Let the heat capacity of water at this temperature is 4.184 J/kg⋅°C and 40mL water has a mass of 40 grams or 0.04kg. If the temperature of the solution increases to 35.32 °C. How much heat is gained by the calorimeter?
You have Q = mc∆T = (0.04 )(4.184 )(35.32 − 30 °C)
= 0.890 kJ
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