Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
17 Cards in this Set
- Front
- Back
deposition
|
gas -> solid
|
|
heat of transition (del H)
|
amt of energy required to complete transition
|
|
when temp doesn't change but phase change, q = ?
|
n * del H
- n (mol) and H (cal/mol) or m * del H |
|
1 cal = what joule
|
4.2 joule
|
|
when a substance absorbs or releases heat, either its temp changes or phase changes but never both. true or false
|
true
|
|
when temp change but phase doesn't change, q = ?
|
q = m*c*del T
-m = mass in gram -c = specific heat (J/g*K) -T = kelvin -q = heat added or released (cal or joule) |
|
the higher specific heat (c), the better the substance what?
|
can hold on to the absorbed heat
|
|
stronger the bond, what happen to specific heat?
|
higher specific heat
ex: CH4 (nonpolar) or CO ( weak dipole force) has weaker bond than CH3OH (H bond) |
|
heat of vaporization > heat of fustion (T or F )
|
T (always)
|
|
during a phase transiton, does the temperature change?
|
NO! (look at the phase transition diagram)
|
|
in phase diagram:
x and y axis are what? |
x = temp
y = pressure |
|
triple point
|
temp and pressure at which all 3 phases exist simulaneouly in equi
|
|
critical point
|
end of liq and gas boundary
|
|
superficial fluid
|
beyond critical point
a substance has both liq and gas ( cannot distinct) |
|
water
|
unlike other, more dense in liq than solid when increase pressure at constant temp
thus it has neg liquid slope in phase diagram |
|
standard state
|
1 atm
298 K or 25 C |
|
STP
|
1 atm
273 K or 0 C |