Chemistry Reactions and Rates Quiz

The study of how fast chemical reactions occur and the factors that influence their speed.

The change in the amount (grams, moles, liters, etc.) of a reactant or product over time.

The process of breaking down aqueous compounds (those dissolved in water) into their individual ions.

Using the coefficients from a balanced chemical equation to compare the rates of consumption or production of different reactants and products.

The volume occupied by one mole of any gas at standard temperature and pressure (STP).

A fixed set of conditions: 0°C (273 K) and 1 atm pressure.

A quantity expressing the number of particles in a substance.

The mass of one mole of a substance.

A chemical reaction where the color of a solution changes over time. This change is monitored by a spectrophotometer, which measures the intensity of light absorbed by the solution.

A reaction that releases heat into the surroundings, causing the temperature to increase.

A reaction that absorbs heat from the surroundings, causing the temperature to decrease.

A container used to measure the heat change in a chemical reaction. It helps isolate the reaction from the environment to accurately measure temperature changes.

A reaction that increases the pressure of a closed container.

A reaction that decreases the pressure of a closed container.

A reaction that produces more gas molecules than it consumes.

A reaction that consumes more gas molecules than it produces.

A method to determine reaction rate by measuring the mass of a solid reactant used up over time. This is suitable when one solid reactant gets consumed, and its mass can be readily measured.

A technique for measuring the rate of a reaction where a gas is produced. The mass of the container and its contents is measured over time, reflecting the escape of the gas.

The change in concentration of a specific ion over time, specifically measured using the molar concentration of that ion.

Ions that remain unchanged throughout a chemical reaction. They are not involved in forming new substances.

Analyzing the change in concentration of a specific ion over time, particularly useful when a substance's concentration is difficult to measure directly.

A technique that utilizes a spectrophotometer to monitor and measure the change in concentration of a specific ion over time, providing valuable insight into the reaction rate.

The process of taking periodic samples of a reaction mixture and analyzing them to determine the concentration of a specific ion using techniques like titration.

A technique for determining the rate of a reaction by analyzing the change in concentration of a specific ion over time, using methods like spectrophotometry or titration.

The rate of a heterogeneous reaction is directly proportional to the surface area of the solid reactant. More surface area allows for more reactant molecules to interact with the other phase.

A substance that inhibits the rate of a chemical reaction without being consumed in the process. Examples include poisons, antibiotics, and sunscreens.

The rate of a chemical reaction is affected by factors like temperature, concentration, and surface area. Each factor influences the rate in a specific way.

Chemical reactions that involve reactants in different physical states (e.g., solid and liquid) are called heterogeneous reactions. The reaction only occurs at the interface, or surface, between these phases.

The rate of a chemical reaction is influenced by the concentration of the reactants. Higher concentration generally leads to a faster reaction rate.

A species that is produced in an earlier step of a reaction mechanism and then used up in a later step. It appears on the right side of one step and on the left side of another step.

The highest energy point on the potential energy diagram for a reaction. It represents the transition state where bonds are breaking and forming.

The step in a reaction mechanism that has the highest activation energy (Ea). It is the slowest step and determines the overall rate of the reaction.

The difference in potential energy between the reactants and the transition state of the rate-determining step.

A reaction mechanism with multiple steps, each with its own activation energy. The steps are shown as bumps on the potential energy diagram.

A species that is present in the starting material (reactants) and is also present in the final product. It does not appear as a reaction intermediate.

A chemical reaction that involves multiple steps, with one step being significantly slower than the others. This slowest step determines the overall rate of the reaction.

The minimum amount of energy required for reactants to overcome the energy barrier and form products. It's like the 'hill' that reactants need to climb to become products.

The energy difference between the reactants and products of a reaction. It tells us whether the reaction releases or absorbs energy.

The minimum amount of energy required for reactants to overcome the energy barrier and form products in the reverse reaction. It's the 'hill' that products need to climb to become reactants.

The energy change for the reverse reaction taking the products back to reactants. It's the negative of ΔH for the forward reaction.