KINETICS/2
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| 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. |
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| INCREASES THE PRESSURE CAUSES ... THE AVERAGE KINETICA ENERGY O PARTICLES TO.REMIAN THE SAME BUT MORE COLLISIONS PER SECOND RATE. |
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| FOR REACTIONS IN SOLUTION AN INCREASE CONC... CAUSES INCREASE INNNER REACTION RATE... HOGHER CONC OF SOLUTION MORE COLLISIONS. |
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| SUCCESSFULCOLLISIONS RESULT IN ... FASTER RATE OF REACTION. |
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| DOUBLE CONC OF ONE REACTANT CAUSES... RATE OF REACTION TO DOUBLE. |
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| A HOMOGENOUS REACTION ...? IS ONE THAT TAKES PLACE IN A SINGLE PHASE. SO FREQ OF COLLISIONS INCREASE. |
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| IF ZINC POWDERED SURFACE AREA INCREASES AND ... HYDROGEN!!! GAS FORMS QUICKER. |
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| HETEROGENOUS CATALYST ARE DESIGNED ... WITH PARGE SURFACE A GREATER CHANCE OF COLLISIONS BETWEEN REACTION MOL AND CATALYST . |
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| INCREASE TEMP MOLS HAVE HIGHER KINETIC ENERGY. SO MORE MOLECUOES POSSESS ACTIVATION ENERGY. AREA UNDER EA LINE BIGGER COZ MORE SUCCESSFUL COLLIONS & FASTER RATE. |
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| INCREASE IN 10 DEGREES CAUSES RATE OR REACTION TO... DOUBLE |
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| AREA UNDER CURVE TO THE RIGHT OF THE ACTIVATION ENERGY ... IS FRACTION OF MOLECULE THAT HAVE ENPUGH ENERGY FOR COLLISION TO BE SUCCESSFUL. |
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| IF RAISED BY 10 DEGREES... THE COLLISION FREQUENCY RAISED BY 1% RESUKTS FROM NO OF MOL WHO POSSESS ACTIV ENERY EQUAL OR GREATER. |
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| HOW DO CATALYST SPEED UP A REACTION... BY PROVIDIBG AN ALTERNATIVE PATHWAY WITH LOWER ACTIVATION ENERGY. |
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| HOMOGENOUS CATALYST ONE.. IN SAME PHASE AS REACTANTS E.G. FE2+ ION CATALYST IN OXIDATION OF IODINE IONS BY PERSULPHATE IONS |
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| THE HOMOGENOUS CATALST WORKS BY REACTING .. WITH ONE OF REACTANTS TO FORM INTERMEDIATE COMPOUND STOLE 4 OXYGENS AND ONE SULPHUR BECOMES FE3+ |
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| THE INTERMEDIATE COMPOUND THEN.. REACTS WITH OTHER COMPOUND TO REFPRM CATALYST & CHANGES I TO SOLID FROM AQ. |
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| POINT OF USING CATALYST AVOIDS... NECCESSITY OF COLLISON BETWEEN 2 NEG COMPOUNDS. |
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| 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. |
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| 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 |
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| HOW CATALYST WORK... CAN BE EXPLAINED USING MAXWELL BOLTMANN DIAGRAM . PRESENCEOF CATALYST DOESNT ALTER THE AVERAGE KINETIC ENERGY. BUT LOWER !!!! ACTIVATION ENERGY. |
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| CATALYS ECAT LARGER AREA UNDER GRAPH. MORE MOLECULES POSSES AMOUNT OF ENERGY. |
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| ENZYMES CATALYST? MORE THAN ONE ACTIVE SITE. SUBSTRATE BINDS LIKE LOCK AND KEY. GLOBULAR PROTIENS. |
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| CHEM BINDING IRREVERSIBLY TO LOCK&KEY.. CAN POISON IT. |
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| BUT ADV OF POISONING ENZYMES... IF BINDS TO ACTIVE SITE FOR HIV E.G. HIV PROTEASE. PREVENT DEVELOPEMENT OF AIDS. |
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| IN HETERGENOUS REACTION INCREASED SURFACE AREA |
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