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24 Cards in this Set
- Front
- Back
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what is meant by the rate of a reaction |
tells us how fast reactants turn into products |
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3 main ways of find out rate of reaction |
-Loss of mass -measuring increasing volume of gas given off -how quickly a solution goes cloudy |
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formula for mean rate of reaction |
quantity of reactant used divided by time |
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how do you calculate the rate of a reaction at a specific time |
-draw tangent to the curve at the asked time -draw a right angled triangle, using the tangent as its longest side -calculate gradient of tangent |
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four main factors which affect the rate of chemical reactions |
-temperature -surface area of solids -concentration of solutions or pressure of gases -presence of catalyst |
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what is collision theory? |
reacting particles do not have to bump into each-other, but need to also collide with enough energy to cause a reaction |
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what is activation energy? |
minimum amount of energy that particles must have before they can react |
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2 factors that make reactions more likely to happen |
-increase frequency of reacting particles colliding with eachother -increase energy they have when they collide |
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what is collision theory used to |
explain how reactant reacts together and why their rate of reaction varies |
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particles collide all the time, but only some collisions lead to __ |
reactions |
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increasing the number of __ in a certain time and the __ of collisions produces __ rates of reactiona |
collisions, energy,faster |
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a __ surface area does not result in more __ with more __, but does increase the __ of collisions |
larger, collisions, energy, frequency |
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What two reasons do collision theory tell you why raising the temp increases the ROR |
-particles collide more often -particles collide with more energy |
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An increased proportion of particles exceeding the activation energy has a greater effect on rate than the increased frequency of collisions |
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Why does increasing the concentration of reactants increase the rate of reaction? |
because there are more particles of the reactants moving around in the same volume of solution. works the same for increasing the pressure of gases |
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define and describe what is a catalyst is used for |
-a substance that changes the rate of reaction -to speed up reactions and reduce energy costs |
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2 examples of a catalyst |
-iron -platinum normally in powders or pelletes |
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2 advantages of catalysts in industry |
-combat climate change (stops carbon dioxide entering atmosphere) -cheaper alternative to energy needed without one |
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the red arrow vs the blue arrow on a reversible reaction |
red= exothermic(in reverse reaction) blue= endothermic (in forward reaction) |
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at equilibrium, the rate of the forward reaction _ the rate of the __ reaction |
equals, reverse |
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what is a equilibrium |
reactants are making products at the same rate of products making reactants. overall, no change in amount of product or reactants. |
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le chateliers principle? |
if u change conditions what happens? |
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haber process |
used to make ammonia |
