Chemistry /Chemistry - Chemical Equilibrium Flashcards Part 2
describe the procedure to investigate the effects of temperture illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction
Using a dropper drop a drop of potassium thiocynate to iron (II) cloride Intially red colour forms due to formation of Fe(CNS)2+ add sln to new test tube in beaker of hot water Temperture increases, equilibrium shiftf to decreasetemperture in endothermic direction to use up heay, reverse reaction favoured to the left ** yellow colour forms due to formation of Fe3+ add some new sln to a beaker of ie cold water temperture decreases. the equilibrium shidtd to increase temperture in the exothermic direction to produce heat red colour forms due to formation of Fe(CNS)+2
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Term
Definition
describe the procedure to investigate the effects of temperture illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction
Using a dropper drop a drop of potassium thiocynate to iron (II) cloride Intially red colour forms due to formation of Fe(CNS)2+ add sln to new test t...
what is the sigificane of the intital red colour in this equilibrium mixture illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction
the equilibrium lies on the right.conc products>conc reactant
explain why changing the pressure has no effect on the equilibrium illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction
all the reactant and produts are in sln, presuress only affecrs equilibrium in gaseous equaltions
give two inductrial applications of Le chatelier’s principle
manfacture of ammonia (Haber process) 2.manufacture of sulfuric acid (contact process)
According to Le Chatelier’s principle, what conditions should be used to maximise the yield of ammonia obtained?
High pressures and Low tempertures
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why are the conditions according to Le Chatelier’s principle to maximise the yield of ammonia obtained not used in practice
high pressures- costly (uneconimical), danger of gasleaks and explosions low temperturs - rate of reaction is two slow
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| Term | Definition |
|---|---|
describe the procedure to investigate the effects of temperture illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction | Using a dropper drop a drop of potassium thiocynate to iron (II) cloride Intially red colour forms due to formation of Fe(CNS)2+ add sln to new test tube in beaker of hot water Temperture increases, equilibrium shiftf to decreasetemperture in endothermic direction to use up heay, reverse reaction favoured to the left ** yellow colour forms due to formation of Fe3+ add some new sln to a beaker of ie cold water temperture decreases. the equilibrium shidtd to increase temperture in the exothermic direction to produce heat red colour forms due to formation of Fe(CNS)+2 |
what is the sigificane of the intital red colour in this equilibrium mixture illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction | the equilibrium lies on the right.conc products>conc reactant |
explain why changing the pressure has no effect on the equilibrium illustate Le Chatelier’s principle by demostrating the effects of both concentration changed and temperture changes on the reaction | all the reactant and produts are in sln, presuress only affecrs equilibrium in gaseous equaltions |
give two inductrial applications of Le chatelier’s principle | manfacture of ammonia (Haber process) 2.manufacture of sulfuric acid (contact process) |
According to Le Chatelier’s principle, what conditions should be used to maximise the yield of ammonia obtained? | High pressures and Low tempertures |
why are the conditions according to Le Chatelier’s principle to maximise the yield of ammonia obtained not used in practice | high pressures- costly (uneconimical), danger of gasleaks and explosions low temperturs - rate of reaction is two slow |
give three uses of ammonia | fertilizers, explosives, cleaning products |
give three uses of sulfuric acid | car batteries detergents paints |
What is meant by the equilibrium constant Kc? | the relationship between the concentration of the reactants and the products for a reaction at equilibrium |
what is the formula for Kc? | Kc = [C][D] / [A][B] ( if the molar ration is not 1, put it as a power on the substance |
What is the only stress that effects Kc | Temperature is the only factor that affects Kc Kc is always constant at constant temperature |
Does concentration effect Kc? | No, Kc is always onstant at constant temperture |
If Kc is greater than 1… | the concentration of products greater than the reactants- equilibrium lies on the right |
If Kc is less than 1.. | the concentration of reactants greater than products- equilibrium lies on the left |
A increase in Kc means…. | the foward reaction is being favoured (More products are being made) |
a decrease in Kc means… | the reverse reaction is beging favoured(more reactants are being made) |
What do the letters in and ICEE table stand for | Intial moles (before reaction begins) Change in moles (use molar ratio) Equilibrium moles (then divide by volume (L) if given Equilibrium molarilty |
What is ment by a type one question | one in which you need to find the value of kc |
What is meant by a type 2 question | one in whcih you know the value of kc and flind somthing else. You introduce kc |