calorimetry. calculating heat q can be found experimentally by measuring the heat flow accompanying...
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Calorimetry
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Calculating Heat
Q can be found experimentally by measuring the heat flow accompanying a reaction
This is done by measuring temperatureThis process is called calorimetry
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Specific Heat (c)
This is amount of heat required to raise the temperature of 1g of a substance 1ºC
Specific heat is different for different substances
A lower specific heat means that it takes a small amount of heat to change the substance’s temperature
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Calculating the Heat Transfer
Heat transfer can be calculated using Q = (c)(m)(Δt)
The specific heat of iron(III) oxide is 0.75 J/g ºC. What is the heat required to increase the temperature of a 1.75 g sample from 25ºC to 380ºC?
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Enthalpy (ΔH)
ΔH is Q at a constant pressureΔH is always the J given off per mole of
reactant (J/mol)
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Example
When 50 ml of a 1.0 M HCl and 50 ml of a 1.0 M NaOH solution are mixed, the temp in a calorimeter increases from 21.0 ºC to 27.5ºC. The total volume of the end solution is 100 ml, its density is 1.0 g/ml, and its specific heat is 4.18 J/gºC. Find the enthalpy change (heat of reaction)?
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Water Chamber Calorimetry
Heat lost by a reaction is gained by a quantity of water in a calorimeter
Heat lost = Heat gainedC(water) = 4.184 J/gºC
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Example
30.0 g of water at 1000C is mixed with 50.0g of water at 150C and allowed to come to thermal equilibrium. What is the final temperature of the mixture?
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Example
In a calorimeter containing 100 g of water at 21ºC, a reaction is carried out in which 3.5 g of NH4NO3 decomposes into N2O and H2O. The temperature raises to 25ºC. Find the heat of reaction.