rates of reaction chemistry
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- Created by: lydia.martiin
- Created on: 11-01-20 16:23
is rusting a fast or slow reaction?
slow
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name two fast reactions
combustion in fireworks and group one metals reacting with water
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what is rate of chemical reaction?
how fast reactants can turn into products
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equations for mean rate of reaction
quantity of reactant used or quantity of product formed \ time
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calculating the rate of reaction on a graph
you do y\x
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steeper the line the..
faster the reaction
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how to draw a tangent
a straight-line that touches the curve at one point and doesn't cross it, then work out the gradient of the tangent
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how must particles collide in order to react?
with sufficient (enough) energy
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how are reactions explained?
by collision theory
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what happens if there are more collisions?
the faster the reaction is
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what is a successful collision?
is a collision that ends in the particles reacting to form products
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how can chemical reactions occur?
only when reacting particles collide with each other and with sufficient energy
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define activation energy
the minimum amount of energy that particles must have to react
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what are the factors affecting rate of reaction?
concentration of reactants in solution, pressure of reacting gas, temperature, surface area of solid reactants, catalysts
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how does a high temperature affect the rate of a reaction?
increases it
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how does temperature work to increase the rate of reaction?
particles move faster as more energy from heat, frequency of collisions increase as particles move faster and collide with more energy the more particles have more energy greater than activation energy to make the reaction happen quicker
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sodium thiosulfate word equation
sodium thiosulfate + hydrochloric acid = sodium choride + sulphur dioxide + sulfur +water
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what happens to the solution with sulfur?
sulfur is a solid precipitate so it turns the solution cloudy
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collision theory as Charlie explained it
as the temp increases the reacting particles have more kinetic energy and therefore the move around more so have more frequent and successful collisions so the rate of reaction increases. the particles must collide with sufficient energy in order rea
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why is activation energy required in collision theory?
to break bonds in the reactants to start the reaction
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what does increasing the concentration do to the rate of reaction?
increases it
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if a solution is more concentrated, what happens to particles ?
means there are more particles knocking about (colliding) in the same volume water (or other solvent) | more particles in the reactants moving around in the same volume of solution
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when pressure of gases increased what happens to particles?
same number of particles occupy a smaller space making more frequent collisions
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what does increasing the concentration or pressure do to the rate of reaction?
increases it as the higher the concentration the quicker the rate of reaction
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how is the rate of a chemical reaction determinded?
by the frequency of successful collisions
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what happens the more crowded together reactant particles are?
more likely they will collide so increased frequency of collisions result in faster reactions
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what do catalysts do to the rate of reactions ?
increase it
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what are catalysts?
a substance that increases the rate of reaction but isn't used up itself in the reaction
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how do catalysts work?
they all work by decreasing the activation energy needed for the reaction to occur, they do this by providing an alternative reaction pathway with a lower activation energy
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example of a biological catalyst?
enzymes
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when using catalysts the industry, how are they useful?
as products can be made more quickly: saving time and money
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what do catalysts reduce the need for?
reduce the need for high temperatures saving fuel and reducing pollution
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what are different catalysts used for?
different reactions
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how are catalysts displayed in an equation?
above the arrow as they're not used up in the reactants
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how can we show how a catalyst has sped up a chemical reaction?
by doing a reaction profile: the curve should be shorter and quicker as it requires less energy to cross the activation energy barrier
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how do catalysts increase the rate of a chemical reaction?
by providing an alternative pathway for the reaction that has lower activation energy
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Other cards in this set
Card 2
Front
name two fast reactions
Back
combustion in fireworks and group one metals reacting with water
Card 3
Front
what is rate of chemical reaction?
Back
Card 4
Front
equations for mean rate of reaction
Back
Card 5
Front
calculating the rate of reaction on a graph
Back
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