chapter 5/6 Flashcards
Boyles law
P1V1=P2V2
Charles’ Law
(V1/T1)=(V2/T2)
Gays Law
(P1/T1)=(P2/T2)
Avagodros Law
(V1/n1)=(V2/n2)
Combined Gas Law
(P1V1/T1)=(P2V2/T2)
Ideal Gas Law
PV=nRT
Daltons Law of Partial Pressures
Pt=Pa+Pb+Pc… ; Pi=XiPt
Root Mean Square
Urms=√ (3RT/M)
in root mean square, what are the units of M and R
M= kg/mol
R= 8.315 J/(mol*K)
Graham’s Law of Diffusion/ Effusion
r1/r2 (rate) =t2/t1 (time) =√ (M2/M1)
Ideal Gas Constant
- 0.08206 (Latm/molK)
- 8.314 (J/mol*K)
atm -> mmHg
1atm = 760mmHg
mmHg -> torr
760mmHg = 760torr
torr -> Pa
760 torr -> 1.013*10^5 Pa
STP
1atm, 273.15K, 1mol=22.4L
initial energy equation
ΔU=q(heat)+w(work)
what does it mean when q (heat) is negative
the heat is moving out/ work is being done by the system
what does it mean when q (heat) is positive
heat is being added/ work is being on done on the system
specific heat equation
q=msΔT
heat capacity equation
q=CΔT
in the heat capacity equation what is C
C=ms ; C in J/degrees celc.
Δ enthalpy, heat energy
ΔHrxn = (qrxn/ mol substance)
what does it mean when enthalpy is +
endothermic reaction
what does it mean when is -
exothermic reaction
specific heat of liquid water
4.184 (J* degreed celc./g)
standard enthalpy of reaction
ΔHrxn= sum of enthalpy of products - sum of enthalpy of reactants
what is the enthalpy when an element is in its most stable state
0 KJ/mol
when is a diatomic element in its most stable state
when it is a gas
when is a metal in its most stable state
when it is a solid
when is mercury its its most stable state
when it is a liquid
