4756027
Description
Flashcards by Dolu Falowo, updated more than 1 year ago
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Created by Dolu Falowo
almost 9 years ago
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| Question | Answer |
| What is an irreversible reaction? | Reactions where the reactants convert to products and where the products cannot convert back to the reactants. |
| What is a reversible reaction? | Where the reactants are converted into products but the products are then converted back into the reactants. |
| What is dynamic equilibrium? | -The concentrations of the reactants and products remain constant. -The forward and reverse reactions are proceeding at equal rates and occur at the same time. |
| What is a homogeneous reaction? Heterogeneous reaction? | When all the reactants and products are in the same physical state. Reactants and products are in different physical states. |
| What conditions of a reaction affect the position of equilibrium? | -Temperature -Pressure -Concentration |
| What is Le Chatelier's Principle? | When a system in equilibrium is disturbed, the position of equilibrium will move in a direction to reduce the effect of the disturbance. |
| How does a change in pressure affect the position of equilibrium? | An increase in pressure at constant temperature shifts the position of equilibrium to the side with a smaller gas volume (less gas moles) A decrease in pressure at constant temperature shifts the position of equilibrium to the side with a larger gas volume (more gas moles) |
| Why are high pressures not used in industrial reactions even when it may produce a high yield? (2) | -It is expensive due to the cost of electrical pumps to apply the pressure and requires expensive strong-walled vessels and expensive valves and other equipment to withstand the pressure. -Higher pressures require safety controls due to the risk of explosion. |
| How does a change in temperature affect the position of equilibrium (if the forward reaction is exothermic)? | -An increase in temperature would shift the position of equilibrium would move from right to left in the direction of the reverse endothermic reaction. -A decrease in temperature would shift the position of equilibrium from left to right in the direction of the forward exothermic reaction. |
| How does a change in temperature affect the position of equilibrium (if the forward reaction is endothermic)? | -An increase in temperature would shift the position of equilibrium from left to right in the direction of the forward endothermic reaction. -A decrease in temperature would shift the position of equilibrium from right to left in the direction of the reverse exothermic reaction. |
| Why are compromise temperatures used? | When a low temperature would increase the yield of a product, but the temperature shouldn't be too low to make the rate of reaction very slow. A compromise temperature is a compromise between rate and yield. |
| How does a change in concentration affect the position of equilibrium (at constant temperature and pressure)? | - The equilibrium will adjust to replace any substance that has been removed or remove any substance that has been added. -Eg. adding more reactants increases the yield of the products. Equilibrium shifts from left to right. Adding more products increases the yield of the reactants. Equilibrium shifts from right to left. |
| How do catalysts affect the position of equilibrium? | -It has no effect of the position of equilibrium -Allows the reaction to get to equilibrium faster. It increases the rate of the forward and reverse reactions equally so equilibrium is attained much more quickly in the presence of a catalyst. |
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