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THERMOCHEMISTRY, https://coggle.it/diagram/YBAMxhfeOnD6ba3M/t/- - Coggle…
THERMOCHEMISTRY
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Systems
Closed Systems
- No reactants or products can escape, only heat can be exchanged freely
Isolated Systems
- Cannot transfer energy or matter with its surroundings
Enthalpy (H)
- Used to quantity the heat flow into or out of and systemin a process that occurs at constant pressure
- ∆H = H (products) - H (reactans)
- ∆H = heat given off absorbed during a reaction at constant pressure
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Calorimetry
- The specific heat (s) of a substance is the amount of heat (q) required to raise the temperature of 1g of a substance by 1℃
- The heat capacity (C) of a substance is the amount of heat (q) required to raise the temperature of a given quantity (m) of the substance by 1℃
- C = ms
Constant-Volume Calorimetry
- qsys = qwater + qbomb + qrxn
- qsys = 0
- qrxn = -(qwater + qbomb)
- qwater = ms∆t
qbomb = Cbomb∆t
- Reaction at Constant V
∆H ≠ qrxn
∆H ∿ qrxn
Constant-Pressure Calorimetry
- qsys = qwater + qcal + qrxn
- qsys = 0
- qrxn = -(qwater + qcal)
- qwater = ms∆t
qcal = Ccal∆t
- Reaction at Constant P
∆H = qrxn
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Hess's Law
- When reactants are converted to products, the changes in enthalpy is the same whether the reaction takes place in one step or in a series of steps.
- (Enthalpy is a state function. It doesn't matter how to get there, only where it start and end)
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