kinetics Flashcards
describe a chemical reaction in terms of Collison theory
reaction occurs when reactant particles collide with sufficient activation energy
define activation energy
minimum energy needed for a reaction to occur and collision to be successful
define rate of reaction
change in quantity of reactant or product over time
explain how an increase in temperature increases rate of reaction
at higher temperatures more particles have energy greater than or equal to activation energy therefore there are more collisions greater than or equal to the activation energy per unit time
explain how an increase in concentration increases rate of reaction
as concentration increases there are more reactant particles per unit volume therefore there are more collisions greater or equal to the activation energy per unit time
explain how increasing pressure increases rate of reaction
as pressure increases there are more particles per unit volume so there are more collisions greater than or equal to the activation energy per unit time
define catalyst
substance that speeds up a chemical reaction without being using up
how does a catalyst increase rate of reaction
provides an alternative reaction pathway with a lower activation energy. More particles have energy greater than or equal to activation energy
Explain how the reaction between hydrochloric acid and sodium
thiosulfate can be monitored
The reaction produces a sulfur precipitate. Time how long it takes for the precipitate to
obscure a cross. Rate = 1 / time
Explain the the reaction between hydrochloric acid and sodium
thiosulfate should only be carried out on a small scale
Toxic sulfur dioxide is a product
Explain why the Maxwell-Boltzman graph starts at the origin
No particles have zero kinetic energy
give the 5 factors that have an impact on the rate of reaction
- increasing the temperature
- increasing the concentration of a solution
- increasing the pressure of a gas reaction
- increasing the surface area of solid reactants
- using a catalyst
