Chemical Reactions and Reaction Stoichiometry

These flashcards cover key concepts related to chemical reactions and stoichiometry as discussed in the lecture.

What are chemical equations used for in chemistry?

To represent chemical reactions on paper.

What is the Law of Conservation of Mass in relation to chemical equations?

Mass is conserved, meaning the mass of reactants equals the mass of products.

How do you balance a chemical equation?

By changing coefficients, not subscripts, starting with elements that are only in one reactant and product.

What does the symbol Δ indicate in a chemical equation?

That heat is needed for the reaction to take place.

What type of reaction involves two or more substances reacting to form one product?

A combination reaction.

In a decomposition reaction, what happens to a single substance?

It breaks down into two or more substances.

What are the typical products of combustion reactions involving carbon and hydrogen?

Carbon dioxide (CO2) and water (H2O).

What is formula weight (FW)?

The sum of the atomic weights of the atoms in a chemical formula.

What does Avogadro’s number represent?

The number of particles in one mole, which is 6.022 × 10^23.

What is the limiting reactant in a chemical reaction?

The reactant present in the smallest stoichiometric amount that limits product formation.

How is percent yield calculated?

By comparing the actual yield to the theoretical yield using the formula: Percent yield = (actual yield/theoretical yield) x 100%.

What is a mole in terms of chemistry?

A mole is the amount of particles found in exactly 12 g of carbon-12.

What factors can contribute to the theoretical yield being different from the actual yield?

Experimental losses, side reactions, or incomplete reactions.