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KINETICS/2

QuestionAnswer
CQN INCREASE PRESSURE BY ... REDUCING VOLUKE OF CONTAINER. PUMPING MORE REACTANT GAS INTO CONTAINER . INCREASED PRESSURE OF GAS PARTICLES PER CM3 SO FREQ PF COLLISONS INCREASES.
INCREASES THE PRESSURE CAUSES ... THE AVERAGE KINETICA ENERGY O PARTICLES TO.REMIAN THE SAME BUT MORE COLLISIONS PER SECOND RATE.
FOR REACTIONS IN SOLUTION AN INCREASE CONC... CAUSES INCREASE INNNER REACTION RATE... HOGHER CONC OF SOLUTION MORE COLLISIONS.
SUCCESSFULCOLLISIONS RESULT IN ... FASTER RATE OF REACTION.
DOUBLE CONC OF ONE REACTANT CAUSES... RATE OF REACTION TO DOUBLE.
A HOMOGENOUS REACTION ...? IS ONE THAT TAKES PLACE IN A SINGLE PHASE. SO FREQ OF COLLISIONS INCREASE.
IF ZINC POWDERED SURFACE AREA INCREASES AND ... HYDROGEN!!! GAS FORMS QUICKER.
HETEROGENOUS CATALYST ARE DESIGNED ... WITH PARGE SURFACE A GREATER CHANCE OF COLLISIONS BETWEEN REACTION MOL AND CATALYST .
INCREASE TEMP MOLS HAVE HIGHER KINETIC ENERGY. SO MORE MOLECUOES POSSESS ACTIVATION ENERGY. AREA UNDER EA LINE BIGGER COZ MORE SUCCESSFUL COLLIONS & FASTER RATE.
INCREASE IN 10 DEGREES CAUSES RATE OR REACTION TO... DOUBLE
AREA UNDER CURVE TO THE RIGHT OF THE ACTIVATION ENERGY ... IS FRACTION OF MOLECULE THAT HAVE ENPUGH ENERGY FOR COLLISION TO BE SUCCESSFUL.
IF RAISED BY 10 DEGREES... THE COLLISION FREQUENCY RAISED BY 1% RESUKTS FROM NO OF MOL WHO POSSESS ACTIV ENERY EQUAL OR GREATER.
HOW DO CATALYST SPEED UP A REACTION... BY PROVIDIBG AN ALTERNATIVE PATHWAY WITH LOWER ACTIVATION ENERGY.
HOMOGENOUS CATALYST ONE.. IN SAME PHASE AS REACTANTS E.G. FE2+ ION CATALYST IN OXIDATION OF IODINE IONS BY PERSULPHATE IONS
THE HOMOGENOUS CATALST WORKS BY REACTING .. WITH ONE OF REACTANTS TO FORM INTERMEDIATE COMPOUND STOLE 4 OXYGENS AND ONE SULPHUR BECOMES FE3+
THE INTERMEDIATE COMPOUND THEN.. REACTS WITH OTHER COMPOUND TO REFPRM CATALYST & CHANGES I TO SOLID FROM AQ.
POINT OF USING CATALYST AVOIDS... NECCESSITY OF COLLISON BETWEEN 2 NEG COMPOUNDS.
HETEROYENOUS CATALYSTS:- ONE IN DIFF PHASE TP REACTANTS E.G. IRON IN HABER PROCESS. N2(G)+ 3H2 --> 2NH3(G) HETEROGENOUS CATALYST PROMOTES REACTION THROUGH ACTIVE SITE. PLACES ON SURAFACE OF CATALYST WHERE REACTANTS CAN BOND.
GASEOUS REACTANTS + ACTIVE SITES= ABSORB REACTANTS . ABSORBED REACTATS ABSORB PRODUCTS. AB PRODUCTS --> GASEOUS PRODUCTS + FREE ACTIVE SITES. FEWER ACTOVE SITES THAN REACTANST MOLECULES SO INCREASE PRESSURE MAKES NO DIFFERNCE ALL ACTIVE SITE OCCUPIED
HOW CATALYST WORK... CAN BE EXPLAINED USING MAXWELL BOLTMANN DIAGRAM . PRESENCEOF CATALYST DOESNT ALTER THE AVERAGE KINETIC ENERGY. BUT LOWER !!!! ACTIVATION ENERGY.
CATALYS ECAT LARGER AREA UNDER GRAPH. MORE MOLECULES POSSES AMOUNT OF ENERGY.
ENZYMES CATALYST? MORE THAN ONE ACTIVE SITE. SUBSTRATE BINDS LIKE LOCK AND KEY. GLOBULAR PROTIENS.
CHEM BINDING IRREVERSIBLY TO LOCK&KEY.. CAN POISON IT.
BUT ADV OF POISONING ENZYMES... IF BINDS TO ACTIVE SITE FOR HIV E.G. HIV PROTEASE. PREVENT DEVELOPEMENT OF AIDS.
IN HETERGENOUS REACTION INCREASED SURFACE AREA
Created by: ufuoma
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