unit 3 KA1 - getting the most from reactants Flashcards
how are industrial processes designed
they are designed to maximise profit and minimise the impact on the environment
what are the factors that influence industrial processes
- availability, sustainability and cost of feedstock(s)
- opportunities for recycling
- energy requirements
- marketability of by-products
- product yield
what are the environment considerations of industrial processes
- minimising waste
- avoiding the use or production of toxic substances
- designing products which will biodegrade if appropriate
what is the mass of a mole of any substance equivalent to
the gram formula mass
what is the molar volume
this is the volume occupied by one mole of any gas at a certain temperature and pressure. the molar volume is the same for all gases at the same temperature and pressure
what data is used when performing calculations
- gram formula mass
- masses
- number of moles
- concentrations and/or volumes of solutions
- molar volumes
- volumes for gases
what is the efficiency with which reactants are converted into the desired product measured in
the percentage yield and atom economy
what is the theoretical yield
this is the quantity of desired product obtained assuming full conversion of the limiting reactant
what is the actual yield
this is the quantity of desired product formed under the prevailing reaction conditions
what does the percentage yield provide a measure of
the degree to which the limiting reagent is converted into the desired product
what equation can be used to calculate the percentage yield
actual yield divided by the theoretical yield times by 100
is it true that given costs for the reactants, a percentage yield can be used to calculate the cost of reactants required to produce a given mass of product?
yes
what does the atom economoy measure
the proportion of the total mass of all starting materials converted into the desired product in the balanced equation
what equation can be sued to calculate the percentage atom economy
the mass of the desired product divided by the total mass of reactants timed by 100
is it true that reactions which have a high percentage yield may have a low atom economy value if large quantities of by-products are formed?
yes
