Pages in this set

Page 1

Preview of page 1
Unit 1notes:
1.3: Formula, equations and amounts of substance
A. Demonstrate an understanding of the terms atom, element, ion,
molecule, compound, empirical and molecular formulae
CompoundA chemical compound is a pure chemical substance consisting of two or more different
chemical elements that can be separated into simpler substances by chemical…

Page 2

Preview of page 2
D. Calculate the amount of substance in a solution of known concentration (excluding titration
calculations at this stage). For example use data from the concentrations of the various species in
blood samples to perform calculations in mol dm3.

Volume in dm3 X concentration in mol dm3 = moles
moles X…

Page 3

Preview of page 3
Avogadro's number is 6.022x1023, in 12grams of Carbon 12 there will be 6.022x1023 atoms of
Carbon as there is precisely one mole of it. A mole is defined as the amount of that substance that
contains the same number of stated elementary units (atoms molecules etc) as the atoms in…

Page 4

Preview of page 4

C. Recall the sign of H for exothermic and endothermic reactions. For example illustrated by the
use of exo and endothermic reactions in hot and cold packs


D. Recall the definition of standard enthalpy changes of reaction, formation, combustion,
neutralization and atomization and use experimental data to calculate energy…

Page 5

Preview of page 5

E. Recall Hess's Law and apply it to calculating enthalpy changes of reaction from data provided,
selected from a table of data or obtained from experiments and understand why standard data is
necessary to carry out calculations of this type

For formation the arrows both point to the element as…

Page 6

Preview of page 6
ii) Deduce the relative atomic mass of an element
iii) Measure the relative molecular mass of a compound




poor, would not read 0/10

Similar Chemistry resources:

See all Chemistry resources »