Topic 4- Lecture 16 Flashcards
Calorimeter
Device used to determine the amount of heat transfer
Heat flow can’t be measured…
Directly
Measure temp before and after and flip sign
Specific heat
Amount of heat it takes to raise the temp of 1 g of a substance by 1 K
Heat lost or gained by a substance
Equation
Δq= m c ΔT Heat lost or gained by a substance Mass of substance Specific heat capacity Change in temperature
Δq of reaction
ΔH of reaction
Heat lost or gained in the experiment
Heat lost or gained in the balanced chemical equation
Hess’s law
Overall change in Enthalpy will be equal to the sum of the Enthalpy changes for the individual steps
Rearrange equations and flip signs of ΔH as necessary, add sums
Standard Enthalpy of formation
Hypothetical value that indicates how much heat would be lost or gained during the formation of one mole of a substance
ΔH°f
°= standard state (298 K, 25°C)
Look values up in table
ΔHrxn= ΣnΔH°f(products) - ΣnΔH°f (reactants)
Sum of
Stoichiometric coefficients
Look up in table
Calorimetry
Lab technique
Measurement of heat transfer