CALORIMETRY Calorimetry: measurement of heat changes

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Presentation transcript:

CALORIMETRY Calorimetry: measurement of heat changes The heat transferred is proportional to the mass of the object (m) specific heat capacity (Cp) temperature change (∆T) Heat has the symbol q and is calculated using q = m∆TCp

Specific heat (s) amount of heat (q) required to raise the temperature of one gram of the substance by one degree Celsius. Water

Specific heat capacity … Heat Capacity (Cp) amount of heat (q) required to raise the temperature of a given quantity (m) of the substance by one degree Celsius. Specific heat capacity … …varies from one substance to another …a measure of how much heat something can “hold” …the amount of heat needed to raise one gram of a substance by one Celsius degree

The specific heat capacity of water is 4.18 J/g∙°C Quantity of heat q = mDTCp The specific heat capacity of water is 4.18 J/g∙°C

q = mDT Cp q =(25.6g)(30.0C) (4.18J/gC) q = 3210 J How much heat is needed to raise the temperature of 25.6 grams of water from 20.0 C to 50.0 C? q = mDT Cp q =(25.6g)(30.0C) (4.18J/gC) q = 3210 J

q = mDTCp = q DT mCp Answer: 6.20 °C What is the final temperature of 27.0 grams of liquid water, initially at 0°C, after it absorbs 700.0 J of energy? q = mDTCp Hint: start by solving for DT. = q DT mCp Answer: 6.20 °C

Dt = Tfinal – Tinitial = 50°C – 940°C = -890°C Ex. How much heat is given off when an 869 g iron bar cools from 940°C to 50°C? s of Fe = 0.444 J/g • °C Dt = Tfinal – Tinitial = 50°C – 940°C = -890°C q = m∆TCp = 869 g x 0.444 J/g • °C x –890°C = -34,000 J