Stoichiometry Quiz

Deals with the quantitative relationships between reactants and products in a chemical reaction
Involves calculating the amounts of substances required for a reaction or produced by a reaction
Key concepts:
- Mole ratios: the ratio of moles of reactants to moles of products
- Limiting reagent: the reactant that is consumed first and limits the amount of product formed
- Excess reagent: the reactant that is present in excess and does not limit the amount of product formed
- Percent yield: the percentage of the theoretical amount of product that is actually formed

Measures the speed at which a chemical reaction occurs
Factors that affect reaction rates:
- Concentration: increasing the concentration of reactants increases the reaction rate
- Temperature: increasing the temperature increases the reaction rate
- Surface area: increasing the surface area of reactants increases the reaction rate
- Catalysts: substances that speed up the reaction without being consumed
- Pressure: increasing the pressure can increase the reaction rate
Methods to measure reaction rates:
- Initial rate method: measures the rate at the beginning of the reaction
- Average rate method: measures the average rate over a period of time
- Graphical method: uses graphs to determine the rate

A process in which a catalyst speeds up a chemical reaction without being consumed
Types of catalysts:
- Homogeneous catalysts: catalysts that are present in the same phase as the reactants
- Heterogeneous catalysts: catalysts that are present in a different phase than the reactants
Characteristics of catalysts:
- They lower the activation energy required for a reaction
- They do not change the equilibrium constant of the reaction
- They can be reused multiple times

Involve the transfer of a proton (H+ ion) from an acid to a base
Types of acid-base reactions:
- Neutralization reactions: acid + base → salt + water
- Acid-base equilibrium reactions: acid + base ⇌ conjugate acid + conjugate base
Key concepts:
- pH: a measure of the acidity or basicity of a solution
- pOH: a measure of the basicity of a solution
- Acid dissociation constant (Ka): a measure of the strength of an acid
- Base dissociation constant (Kb): a measure of the strength of a base
- Buffer solutions: solutions that resist changes in pH when an acid or base is added

Deals with the quantitative relationships between reactants and products in a chemical reaction
Involves calculating the amounts of substances required for a reaction or produced by a reaction
Key concepts include:
- Mole ratios: the ratio of moles of reactants to moles of products
- Limiting reagent: the reactant that is consumed first and limits the amount of product formed
- Excess reagent: the reactant that is present in excess and does not limit the amount of product formed
- Percent yield: the percentage of the theoretical amount of product that is actually formed

Measures the speed at which a chemical reaction occurs
Factors that affect reaction rates:
- Concentration: increasing the concentration of reactants increases the reaction rate
- Temperature: increasing the temperature increases the reaction rate
- Surface area: increasing the surface area of reactants increases the reaction rate
- Catalysts: substances that speed up the reaction without being consumed
- Pressure: increasing the pressure can increase the reaction rate
Methods to measure reaction rates:
- Initial rate method: measures the rate at the beginning of the reaction
- Average rate method: measures the average rate over a period of time
- Graphical method: uses graphs to determine the rate

A process in which a catalyst speeds up a chemical reaction without being consumed
Types of catalysts:
- Homogeneous catalysts: catalysts that are present in the same phase as the reactants
- Heterogeneous catalysts: catalysts that are present in a different phase than the reactants
Characteristics of catalysts:
- Lower the activation energy required for a reaction
- Do not change the equilibrium constant of the reaction
- Can be reused multiple times

Involve the transfer of a proton (H+ ion) from an acid to a base
Types of acid-base reactions:
- Neutralization reactions: acid + base → salt + water
- Acid-base equilibrium reactions: acid + base ⇌ conjugate acid + conjugate base
Key concepts:
- pH: a measure of the acidity or basicity of a solution
- pOH: a measure of the basicity of a solution
- Acid dissociation constant (Ka): a measure of the strength of an acid
- Base dissociation constant (Kb): a measure of the strength of a base
- Buffer solutions: solutions that resist changes in pH when an acid or base is added

Increasing the concentration of reactants increases the reaction rate, as more reactant particles are available for collisions.
A rise in temperature increases the reaction rate by providing more energy for collisions between particles, thereby increasing the frequency of successful collisions.
Increasing the surface area of reactants increases the reaction rate by providing more sites for collisions to occur.
Adding a catalyst increases the reaction rate by lowering the activation energy required for the reaction, allowing more particles to react.
Increasing the pressure increases the reaction rate by forcing particles closer together, increasing the frequency of collisions.

The frequency of collisions between reactant particles affects the reaction rate, as more frequent collisions increase the likelihood of successful reactions.
The activation energy required for a collision to result in a reaction affects the reaction rate, as higher activation energies reduce the frequency of successful reactions.
The orientation of collisions between reactant particles affects the reaction rate, as only certain orientations result in successful reactions.

The slowest step in a reaction mechanism determines the overall reaction rate, as it is the step that limits the rate of the overall reaction.
The rate-determining step is the step with the highest activation energy, requiring more energy for the reaction to occur.

A rate law describes the relationship between the reaction rate and the concentrations of reactants, providing a mathematical representation of the reaction.
The rate constant is a constant that describes the relationship between the reaction rate and the concentrations of reactants.
The order of reaction is the power to which the concentration of a reactant is raised in the rate law, describing the effect of concentration on the reaction rate.

The instantaneous rate is the rate of reaction at a specific instant in time, providing a snapshot of the reaction rate.
The average rate is the rate of reaction over a specific period of time, providing an overall view of the reaction rate.
The initial rate is the rate of reaction at the beginning of the reaction, often used as a benchmark for comparison with later stages of the reaction.