Mass calculations for SQA Higher Chemistry
This page covers the following topics:
1. Theoretical mass
2. Atom economy
Due to incomplete reactions, when experiments are carried out there is not a 100% yield of products. The theoretical yield is the amount of product you could produce theoretically. The percentage yield is a measure of the amountthe actual yield you get from an experiment.
Atoms are not gained or lost in a chemical reaction, some atoms from the reactants end up in the product, and some in by-products. The atom economy of a reaction expresses how efficiently a reaction makes use of reactant atoms, i.e. how much product is creating in comparasion to by-product. Atom economy is a percentage, thus the highest it can possibly be is 100%.
What is the definition of atom economy?
A measure of the amount of starting elements/compounds that end up as useful products.
3 g of C₃H₇OH has reacted with an excess of CH₃COOH (Ar = 60 g/mol) to give 1.8 g of C₃H₇OOCCH₃ (Ar = 102 g/mol) and some water, what is the actual yield of this reaction?
Actual yield is the experimental mass of the product.
What is the theoretical yield?
The maximum possible mass of product you could produce from a reaction
What is the actual yield?
The actual yield is the final mass of product produced in a reaction.
the actual mass of product yielded in a reaction
The percentage yield of the production of Cu from 6.5 g of Zn is 75%. Use the reaction equations provided to find the mass of copper produced.
Zn + CuSO₄ → ZnSO₄ + Cu
1 : 1 mole ratio
6.5 ÷ 65.38 = 0. 099 mol
0.1 × 63.55 = 6.32 g
6.4 × 0.75 = 4.74 g
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