Specific Heat Calorimetry.

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Presentation transcript:

Specific Heat Calorimetry

Calculating Heat Transferred Q = mCT Q = amount of heat transferred m = mass of substance C = specific heat capacity of the substance. T = temperature change = Tfinal – Tinitial

Calorimeter source

Another calorimeter source source

Heat in Chemical Reactions Changes in heat energy are measured by The “universe” is contained in a styrofoam cup. The “enviroment” is the water.**** The “system” is whatever we put in the water. calorimetry

Energy lost = Energy gained Calorimetry Energy lost = Energy gained Difficult to monitor the “system.” Easy to monitor the “environment” – that’s the water! Energy lost/gained by environment = Energy gained/lost by system

Exothermic – the temperature of the environment increased. Calorimetry 10 grams of NaOH are dissolved in 100 g of water. The temperature of the water increases from 22C to 30C. Was the dissolving process endothermic or exothermic & how do you know? Exothermic – the temperature of the environment increased.

Dissolving What’s happening when the NaOH dissolves? Add H2O Close together. Not interacting with H2O. Pulled apart & interacting with H2O.

Calorimetry Q = mCT Q = energy (joules) M = mass (grams) Calculate the energy released by the NaOH in the previous problem as it dissolved in the water. Energy lost by NaOH = Energy gained by water. Easier to calculate from H2O perspective. Q = mCT Q = energy (joules) M = mass (grams) C = specific heat capacity (Table B) T = temperature change = Tf - Ti

Calorimetry & Q = mCT The temperature of the water increased from 22C to 30C. 30C -22C = 8C = T What mass? Well, the temperature change was for the water, so you want the mass of the water. m = 100 g. Same goes for specific heat capacity. We’re going to calculate the heat absorbed by the water. CH20 = 4.18J/g

Q = mCT Q = 100 g X 4.18 J/g X 8C Q = 3344 Joules.

Expressing Heat Changes The heat content of a system at constant pressure is the same as a property called Heat released or absorbed (Q) by a reaction at constant pressure is the same as a change in enthalpy (rH), therefore, Q = rH. ENTHALPY