Unit 1 Section 5- Redox and Equilibria Flashcards
What happens when the concentration of a product is decreased?
Equilibrium will shift to the right in order to produce more product and oppose its removal
What happens when the concentration of a reactant is decreased?
Equilibrium will shift to the left in order to produce more reactant and oppose its removal
What will happen when the concentration of a reactant increases?
Equilibrium will shift to the right in order to use up some of the reactant and oppose the extra reactant
What happens when the temperature increases during a reaction?
Equilibrium will shift left in the endothermic direction in order to oppose the increase in temperature
What happens when the temperature of a reaction decreases?
Equilibrium will shift right in the exothermic direction in order to oppose the temperature decrease
What happens when the pressure of a reaction increases?
Equilibrium will shift right to favour a decrease in pressure by favouring the reaction that produces less moles of gas
What happens when the pressure of a reaction decreases?
Equilibrium will shift left to favour an increase in pressure by favouring the reaction that produces more moles of gas
What happens to the equilibrium when a catalyst is added to a reaction?
There is no effect on the equilibrium but it will speed up the rate at which equilibrium is reached as it speeds up both reactions by the same amount
How do you calculate the partial pressure of a gas?
Mol A/ total moles = mol fraction of A
Mol fraction x total pressure
How does increasing concentration affect the rate of a reaction?
It increases the number of particles per cm3. The particle collision frequency increases. Particles energy remains unaffected
How does increasing pressure affect the rate of reaction?
It increases the number of particles per cm3. The particle collision frequency increases. Particle energy remains unaffected
How does increasing the surface area affect the rate of reaction?
It exposes more particles to collision. There will be more collisions per second
How does increasing temperature affect the rate of reaction?
At higher temperatures the particles move faster so they collide more frequently. A higher percentage of the molecules have the activation energy or more so there is a higher proportion of successful collisions
What is the equation for rate?
Change in temperature/ time
