[CHEM] Unit 8- Matter and Heat Flashcards
The process of going from S to G is ___ and from G to S is ___
Sublimation, deposition
These two elements sublime under normal circumstances:
I2 (iodine) and CO2 (carbon dioxide)
To convert from K to C, you ___ 273
SUBTRACT
To convert from C to K, you ___ 273
ADD
Temperature is the measure of the average ____
Kinetic energy
Kinetic energy is related to the ___
The speed of the motion of particles
A triple point is where ___
All the lines meet; all three phases are in equilibrium together
Above the critical point/temperature, it is ___
Impossible to condense a gas into liquid by just increasing the temperature- additionally, above this point gas and liquid are indistinguishable from each other
In a phase diagram, if the solid is MORE dense than liquid, it will have a ___ curve
Positive
In a phase diagram, if the solid is LESS dense than liquid, it will have a ___ curve
Negative
Endothermic is ____
Putting heat in (heat is a reactant)
Exothermic is ___
Taking heat out (heat is a product)
Boiling is ___, freezing is ___
Endothermic, exothermic
In a heating or cooling curve chart (H/C curve), the flat areas are the ___
Phase changes
During phase changes, only ___ energy changes
Potential
In a H/C curve, the diagonal regions are ___
Single phases warming or cooling
During cooling or warming, only ___ energy and ___ changes
Kinetic, temperature
T/F: The freezing point of a substance is the same as the melting point
T
T/F: The boiling point of a substance in a cooling curve IS NOT the point where the gas begins to condense
F- the BP IS the point
Equation for energy change in boiling: q(___)=m(___)Hv(___)
Heat (in Joules), mass (in grams), and the heat of vaporization (tells you how much heat is needed to boil 1 gram at its BP)
For water, the heat of vaporization is ___ J(g)
2260
Equation for energy change in melting: q(___)= m(___)Hf(___)
Heat, mass, and heat of fusion (jow much heat is needed to melt 1 gram at its BP)
For water, the heat of fusion is ___J(g)
334
Equation for energy change in the diagonals (single phase): q(___)= m(___)c(___)∆T(___)
Heat (in Joules), mass (in grams), specific heat [capacity] (how much energy/heat is takes to raise the temp of 1 gram sample by 1C), change in T (always final-initial)
For specific heat capacity, the unit is ___
J/g°C
The specific heat capacity of water in the solid phase is ___ J/g°C
2.09
The specific heat capacity of water in the liquid phase is ___ J/g°C
4.18
The specific heat capacity of water in the gas phase is ___ J/g°C
1.84
