2C4H10 + 1302 ▯8C02 + 10H20
10g = .14 mole
Given: 10g of C4H10
Question: How much C02 formed?
Under same constant pressure and temperature, volume to mole ratio will be constant.
Periodicity # of neutrons is mass – atomic number
Noble gases don’t react as 8 valence electrons
CORE ELECTRONS= ATOMIC NUMBER – VALENCE ELECTRONS (what column it
99.9% of space in atom is empty…orange in a hockey rink (example)
diatomic molecules – almost never exist by themselves
mass percent = molecular mass= 8 grams, 48 grams of carbon, 1 mole of C4H10 Mass
percent of carbon = 48/58
Mass of molecule/mass of total molecules
What limits the combustion switch to moles and compare ratio…larger ratio is the
5 moles of C4H10 ▯