Experiment 3 CHM1032L
A 28.25 g sample of a metal, initially at 100.0⁰C, is mixed with 100. mL of water,initially at 24.5⁰C, in a coffee cup calorimeter. The water/metal mixture reaches an equilibrium temperature of 28.0⁰C. Calculate the specific heat of this metal.
.172
Sh of liquid water
1.00 cal/g •°C
boiling water temperature
100 degrees Celsius
How much heat must be added to 50.0 g of water to raise the temperature of the water from 24.5⁰C to 36.5⁰C? The SH of liquid water is 1.00 cal/g•⁰C.
600. cal
endothermic reaction
A reaction that ABSORBS energy in the form of heat
exothermic reaction
A reaction that releases energy in the form of heat
Heat lost by the ______ = heat gained by the _____
Heat lost by the ___metal___ = heat gained by the __water___
endothermic reaction formula
Reactant + heat --> product
SH of a metal during a metal/water mixture
SH m = (mass of wtr x SH of wtr x 🔺T of wtr) / ( mass of metal x 🔺M)
sign of heat change for an exothermic reaction and endothermic
exo: -, increase temp endo: + , decrease temp
t or f : the specific heat (SH) of a substance is the amount of heat that is needed to raise the temperature of one gram of the substance by 10 degree Celsius
false
true or false: Reactions that evolve heat are known as endothermic reactions and the heat evolved is given by convention, a negative sign.
false
moles of salt formula
mass of salt/ formula weight of salt
the ______ temperature reached by the water/metal mixture after mixing will be taken as the equilibrium temperature.
maximum
heat of solution formula ( 🔺Hs )
q/ (# of moles of solute) _______________ in data sheet: 🔺Hs = (100. + A)(D-E)/C A= mass of salt D= initial T of water E= final T of water C= moles of salt
formula of heat gained or lost
q= mass x SH x 🔺T the queen took a mass shat 🔺T = T final - T initial
exothermic reaction formula
reactants --> products + heat
Specific heat
the amount of heat that is needed to raise the temperature of one gram of the substance by one degree Celsius
