This document discusses the concept of atom economy, which is a measure of efficiency in chemical reactions. It is defined as the ratio of the total weight of atoms in the products to the total weight of atoms in the reactants. A higher atom economy means more of the reactants are incorporated into the desired products and less is wasted. The document provides an example reaction and calculations to show how atom economy is determined. It explains that both yield and atom economy should be considered when designing green chemical processes in order to minimize waste.
green chemistry : is the design of chemical products and process that reduce the eliminate the use and generation of hazardous substances
atom economy : the maximum amount of all raw material end up into desired products and a minimum amount of waste product is produced. the mass of product that we want as a% of the mass of all products
examples :
importance :
type of reactions
t
This slide show. gives the total knowledge of green chemistry and its applications in various fields. It also describes the essentiality of green chemistry and its role in decreasing pollution
Power Point Presentation on GREEN CHEMISTRY
(info on pollution, causes and its prevention)
Friends if you found this helpful please click the like button. and share it :)
green chemistry : is the design of chemical products and process that reduce the eliminate the use and generation of hazardous substances
atom economy : the maximum amount of all raw material end up into desired products and a minimum amount of waste product is produced. the mass of product that we want as a% of the mass of all products
examples :
importance :
type of reactions
t
This slide show. gives the total knowledge of green chemistry and its applications in various fields. It also describes the essentiality of green chemistry and its role in decreasing pollution
Power Point Presentation on GREEN CHEMISTRY
(info on pollution, causes and its prevention)
Friends if you found this helpful please click the like button. and share it :)
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1. Definition
Green chemistry is “the design of
chemical products and processes
that reduce or eliminate the use and
generation of hazardous substances”
2. 12 Principles of Green Chemistry
......
…..
7. Maximize atom economy
What’s atom economy ?
3. ATOM ECONOMY
Barry Trost, Stanford University
“Because an Atom is a Terrible Thing to
Waste”
A Measure of the Efficiency of a Reaction
How many of the atoms of the reactant are
incorporated into the final product and how
many are wasted?
4. All the designers of chemical processes
want to make the maximum amount of
product they can from a given raw
material.
It is possible to calculate how successful
one of these processes is by using the
idea of yield.
5. Mass of product actually made
% Yield = __________________________
X 100
Maximum mass of product that
could be
made(theoretical yield)
6. In a chemical synthesis of calcium oxide, calcium
carbonate is roasted in an oven. The equation for the
reaction is:
CaCO3(s)→ CaO(s) + CO2 (g)
MMr: 100 56 44
The maximum mass of CaO that could be
made from 1mol of CaCO3 (=100g) is 56 g
7. If 50 kg calcium carbonate is used and 21 kg
calcium oxide is made, what is the percentage
yield of the reaction?
theoretictal yeld = 28g calcium oxide
21kg
_____________
% yeld = x 100 = 75%
28 kg
8. ATOM ECONOMY
The idea of yield is useful, but from a Green
Chemistry and sustainable development perspective,
it is not the full picture. This is because yield is
calculated by considering only one product.
One of the key principles of Green Chemistry is that
processes should be designed so that the maximum
amount of all the raw materials ends up in the
product and a minimum amount of waste is
produced
9. ATOM ECONOMY
A reaction can have a high percentage
yield but also make a lot of waste product.
This kind of reaction has a low atom
economy.
Both the yield and the atom economy have
to be taken into account when designing a
green chemical process.
10. Look again at the reaction you considered
CaCO3(s)→ CaO(s) + CO2 (g)
MMr: 100 56 44
If we split up the formulae, we can look at what
happens to each atom in the reaction. The atoms
shown below in bold end up in the product we
want, the rest do not:
Waste
Ca C O O O → Ca O COO
box
1C 2O
11. From the original atoms, one C atom and two O
atoms are wasted – they are not in the
final,useful product.
Green chemists define atom economy as
FW of atoms utilized
% Atom Economy = ____________________ x 100
FW of all reactant
So for this example,
56 (FW CaO)
_______________
% Atom Economy = x 100 %A.E= 56%
100 (FW CaCO3)
12. ATOM ECONOMY IN A SUBSTITUTION REACTION
This kind of reaction has a low atom economy.
CH3CH2CH2CH2OH + NaBr +H2SO4→CH3CH2CH2CH2Br + NaHSO4+ H2O
1 2 3 4 5 6
0.0108mole 0.0129 0.0200 0.0108 mole
0.08g 1.33 2.0 1.48 g (theoretical yield)
limiting reagent
Suppose the actual yield is 1.20 g of compound 4.
%yeld= (1,20g/1,48g) x100 = 81%
13. CH3CH2CH2CH2OH + NaBr +H2SO4→CH3CH2CH2CH2Br + NaHSO4+ H2O
1 2 3 4 5 6
ATOM ECONOMY TABLE
% Atom Economy = (FW of atoms utilized/FW of all reactants)
X 100 = (137/275) X 100 = 50%
FW = formula weight
14. Step-by-step: How to calculate atom economy
Step 1. Write out the balanced equation
Step 2. Calculate the FW of each of the reactants
(remember to account for stoichiometric coefficients)
Step 3. Calculate the FW of the product (remember to
account for stoichiometric coefficients)
Step 4. Apply the formula
FW of all atoms utilized
______________________
% atom economy = x 100
Total FW of all reactants
If one considers the above reaction where a total of 4.13 g of reactants (0.8 g of 1-butanol, 1.33 g of NaBr and 2.0 g of H2SO4) was used, and that at best this reaction will only yield 1.48 g of the desired product, the question might be asked "what happens to the bulk (4.13 g -1.48 g = 2.7 g) of the mass of reactants?". The answer is they end up in side products (NaHSO4 and H2O) that may be unwanted, unused, toxic and/or not recycled/reused. The side products are oftentimes treated as wastes and must be disposed of or otherwise treated. At best only 36% (1.48 g/4.13 g X 100) of the mass of the reactants end up in the desired product. If the actual yield is 81% then only 29% (.81 X .36 X 100) of the mass of the reactants actually ends up in the desired product!
In the equation we have illustrated the atom economy of this reaction by showing all of the reactant atoms that are incorporated into the desired product in green,while those that are wasted are shown in red. Likewise the atoms of the desired product are in green and the atoms composing the unwanted products are in red. Table 3 provides another view of the atom economy of this reaction. In columns 1 and 2 of this table, the formulas and formula weights (FW) of the reactants are listed. Shown in green (columns 3 and 4) are the atoms and weights of the atoms of the reactants that are incorporated into the desired product (4), and shown in brown (columns 5 and 6) are the atoms and weights of atoms of the reactants that end up in unwanted side products. Focusing on the last row of this table it can be seen that of all the atoms of the reactants (4C, 12H, 5O, 1Br, 1Na and 1S) only 4C, 9H, and 1Br are utilized in the desired product and the bulk (3H, 5O, 1Na, 1S) are wasted as components of unwanted products. This is an example of poor atom economy! continua nella prossima slide
The percentage atom economy can be calculate by taking the ratio of the mass of the utilized atoms (137) to the total mass of the atoms of all the reactants (275) and multiplying by 100. As shown below this reaction has only 50% atom economy. % Atom Economy = (FW of atoms utilized/FW of all reactants) X 100 = (137/275) X 100 = 50% Thus at best (if the reaction produced 100% yield) then only half of the mass of the reactants would be incorporated into the desired product while the rest would be wasted in unwanted side products.
