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7. How far? How fast? - Coggle Diagram
7. How far? How fast?
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7.2 Rate of reaction
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Temperature
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Study the effect of temp on the rate of production of gas
Ex) sodium thiosulfate and hydrochloric acid.
Sodium thiosulfate + hydrochloric acid -> sodium chloride + sulfur + sulfur dioxise + water
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the speed of reaction is inversely proportional to the time taken for the reaction to finish.
- rate of reaction increases, when the time decreases.
rate of reaction != 1/time
7.3 Catalysts
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collision theory
If a solid is broken into smaller pieces due to the collision, there is more surface exposed.
- the more collision takes place, the more chance of a reaction
Concentrated: more reactant particles in a given volume -> more collision
- More concentrated the solution, faster speed of reaction.
ex) concentrated acid reacts more vigorously with a piece of magnesium ribbon
Gas - As the pressure increases, the rate of reaction increases.
temperature - raised temp -> particles move faster -> more collision (more chance of reaction).
- Higher the temperature, the faster the reaction.
Raised Temp -> particles to have more energy -> increases the chance that a collision will result in bonds in the reactants breaking and forming the bonds to make the products.
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