Chapter 3 Amount of Substances Flashcards
what is the mole equation for solids and liquids
moles (mol) = mass (g) / Mr
what is the concentration equation for substances
concentration (moldm^-3) = moles (mol) / Volume (dm^3)
what is the moles equation for gases at RTP
moles (mol) = Volume (dm^3) / molar gas volume (24dm^3)
what is the gas equation
Pressure (Pa) x Volume (m^3) = moles (mol) x Gas Constant (8.314) x Temperature (K)
what is the percentage yield equation
Percentage Yield = (Actual Yield / Theoretical Yield) x 100
what is the Atom Economy equation
(molar mass of desired products / molar mass of all products) x 100
What is Avogadro’s Number
6.02 x 10^23
What is Avogadro’s Number (definition)
a number that is used to scale up to find moles
How many atoms are in one mole of an element
6.02 x 10^23 atoms
What is a mole
A unit that measures amounts in terms of number of atoms
What is Ar
Relative atomic mass
What is Mr
Relative Molecular mass
what is the empirical formula
the formula of a molecule in its simplest ratio C1H3
what is the molecular formula
the formula of a molecule in its actual ratio C2H6
how much is 1dm in cm
10cm
how much is 1dm^3 in cm^3
1000cm^3
How do you convert from Celsius to Kelvin
take you Celsius reading and add 273. You should never have a negative Kelvin reading
how do you calculate % difference for experiments
% difference = [(actual - expected) / Actual] x 100
how do you calculate % error for experiments
% error = (error / reading) x 100
what is a procedural error
an error in what you did during the experiment or in the method
what is a precision error
an error in the equipment
what are the three Ideal gas laws
> Size/volume of the gaseous atoms are negligible
No attraction between the atoms
Not at low temperature and high pressure conditions
what is Room Temperature
20 C
what is Room Pressure
101 KPa
