Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state.

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Presentation transcript:

Thermochemistry: The study of heat changes that occur during chemical reactions and physical changes of state

Energy Heat (q) = Form of energy always flows from a warmer object to a cooler object Law of Conservation of Energy – Energy is neither created nor destroyed

Heat (q) The unit is the joule (J) or calorie (cal) 1 calorie = 4.186 J 1 Calorie (food) = 1000 cal (science) = 1 kcal

Specific Heat (C) Specific Heat (C) – the amount of heat required to raise 1 gram of a substance by 1C Specific heat is an intensive property, Every substance has its own specific heat Ex. Water = 4.18 J/(g ∙ ºC) Glass = 0.50 J/(g ∙ ºC)

Specific Heat Units for Specific Heat ( C ) = J / g ● ºC (joules per gram degree Celsius) Equation for Specific Heat: C = q / (m Δ T) This equation can be rearranged to solve for heat (q) q= CmΔT C = specific heat; q = heat; m = mass and ΔT = change in temperature (Tf – Ti)

Specific Heat A 10.0 g sample of iron changes temperature from 25.0C to 50.4 C while releasing 114 joules of heat. Calculate the specific heat of iron.

Example C= q/ (m∆T) C=114 J/ (10.0 g x 25.4°C) c = 0.449 J/g C

Another example If the temperature of 34.4 g of ethanol increases from 25.0 C to 78.8 C how much heat will be absorbed if the specific heat of the ethanol is 2.44 J/g C

Another example First, rearrange the specific heat formula to solve for heat q = CmT q = (2.44 J/g°C)(34.4g)(78.8°C – 25.0°C) q = 4520 J

Yet another example 4.50 g of a gold nugget absorbs 276 J of heat. What is the final temperature of the gold if the initial temperature was 25.0 C & the specific heat of the gold is 0.129J/g C

Yet another example C= q/ (m∆T); rearrange to find ∆T = q / (C x m) ∆T = 276 J / (.129 J/g°C x 4.50 g) T = 475C T = Tf-Ti 475 = Tf - 25 Tf = 500 C

Phase Changes How many joules are required to raise the temperature of 200.0 g of ice at -10.0˚C to 50.0˚C? Cice = 20.9 J/g ˚C Cwater = 4.184 J/g ˚C ΔHfusion = 6.01 kJ/mol Answer: 150.4 kJ

How much energy is required to bring 45 g of benzene from - 10˚C to 70˚C? (hint: draw a heating curve to help)

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