Reactivity 2.1—How much? The amount of chemical change Flashcards
Coefficient
A number placed before each chemical species indicating it’s relative amount in a chemical equation.
Steps to formulating a Chemical Equation
- Write the word equation with reactants on the left and products on the right.
- Convert reactants and products into chemical formulas.
- Balance the equation
- Add state symbols
Limiting reactant
The substance which is completely consumed in a chemical reaction and determines the yield of the product formed.
Excess reactant
The reactant which is still remaining after the reaction has taken place.
Theoretical yield
The maximum amount of product that could be obtained from a chemical reaction, assuming all reactants are completely converted into products.
Percentage yield
The experimental yield actually produced by the reaction compared to the theoretical yield, expressed as a percentage.
Percentage yield formula
percentage yield = experimental yield / theoretical yield x 100
By-products
An additional product that is formed alongside the desired product during a chemical reaction.
Atom economy
A measure reaction efficiency which compares the total mass of reactant atoms which end up as desired products, represented as a percentage.
Green Chemistry
The field of chemistry which focuses on creating chemical processes and products that are sustainable and environmentally friendly.
What is a chemical equation and what does it include?
A chemical equation represents a chemical reaction, detailing the chemical formulas of the reactants and products, which are separated by an arrow. It also includes state symbols for each species involved.
What information does a balanced chemical equation provide and how is it utilized in data conversion?
A balanced chemical equation displays mole ratios of species via coefficients, enabling conversion of mass, volume, or concentration from one species to another by applying these ratios after converting to moles.
What causes differences between theoretical and percentage yield in chemical reactions?
Differences arise due to incomplete reactions, alternative reactions taking place, loss during transfer of reactants or products, and impurities in the reactants.
