Gen Chem 1 Formulas

1 kg = ? lbs

2.205 lbs

1 mile = ? km

1.609 km

1 in = ? cm

2.54 cm

coverting C to K

K = C + 273.15

converting F to C

C = (F-32)(5/9)

calculating density

d=m/v

solid to liquid

melting

solid to gas

sublimation

liquid to solid

freezing

gas to solid

deposition

liquid to gas

gas to liquid

condensation

4 outlines of Dalton's Atomic Theory

1. Atom is the smallest indivisible particle.
2. Atoms of the same element are identical in mass, but different from those of other elements.
3. Atoms combine in whole number ratios to form compounds.
4. Atoms are neither created nor destroyed.

calculating the number of neutrons

atomic mass - number of protons

SO3

sulfur trioxide; do not use the mono- prefix in first element

N2O4

dinitrogen tetroxide

AlBr3

aluminum bromide

ammonium

NH4+

nitrite

NO2-

nitrate

NO3-

sulfite

SO3-2

sulfate

SO4-2

hydroxide

OH-

7 diatomic elements

hydrogen, nitrogen, fluorine, oxygen, iodine, chlorine, bromine

mole to molecules

1 mole = 6.022x10^23 molecules

percent yield

actual yield/theoretical yield

reduction is ___

gain of electron

oxidation is ____

loss of electron

mmHg to atm

1 atm = 760 mmHg

torr to atm

1 atm = 760 torr

pascal (Pa) to atm

1 atm = 1.01325x10^5

universal gas constant (R)

0.08206 Latm/molK

ideal gas law

PV=nRT

stp

22.4 L per 1 mol at 0C and 1 atm

gas density equation

PM(molar mass)=dRT

average kinetic energy/urms

sqrt(3RT/M)

rate and molar mass known

rx/ry = sqrt(my/mx)

change in energy with heat and work

delta E = q+w

work

P(delta V)

heat capacity and energy equation

q=nC(delta T)

methane

CH4

ethane

C2H6

propane

C3H8

butane

C4H10

change in energy; wavelengths

E = hv