Gas is formed.Collected by gas syringe to measure volume of gas produced. Look at reaction in mass to see the rate of reaction - mass is lit over a period of time
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Rate of Reaction: Magnesium strips
Time taken for Mg to disappear. The mg reacts with dilute HCL, Faster it dissolved, faster it disappears
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Rate of Reaction: Sodium thiosulfate and acid
Clear to CLOUDY Solution // measure time taken for cross to disappear underneath on tile due to cloudiness
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Rate of reaction formals [2]
Amount of reactant used/ Time Amount of reactant produced / Time
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When do chemical reactions occur
when the reacting particles collide with enough energy, the minimum amount of energy required is the activation energy
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Changing rate of reaction factors
Temp, concentration, pressure, surface area
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Concentration
increase concentration = faster rate of reaction. Increasing concentration increases the frequency of SUCCESSFUL collisions so the rate of reaction increases as particles are packed more closely together
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Temperature
Raising the temp = gives the particles MORE ENERGY. This increases the speed of the particles so they collide more FREQUENTLY and more ENERGETICALLY with the activity energy
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Pressure
Increasing pressure reduces sp[ace for particles so the particles get closer together ... Increases frequency of SUCCESSFUL collisions which increases rate of rate of reaction
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Surface area
same concentration concentration and temp (control variables) Increasing surface area increases frequency of collisions
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What is a catalyst
substances which speed up chemical reactions without being changed or used up during the reaction.
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Example of use of catalyst
Hydrogen peroxide --- water + oxygen // This reaction is VVVVV SLOW!!
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How to speed up this reaction of hydrogen peroxide
Use manganese oxide catalyst -- Oxygen is produced much more rapidly
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Other cards in this set
Card 2
Front
Rate of Reaction: Magnesium strips
Back
Time taken for Mg to disappear. The mg reacts with dilute HCL, Faster it dissolved, faster it disappears
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