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23 Cards in this Set
- Front
- Back
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purpose |
to determine the rate and order of the reaction for the decomposition of hydrogen peroxide (H2O2) |
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method |
-added KI and distilled water to flask and swirled in bath water to attain the same temp -connect gas pressure sensor to lab quest -added H2O2 to flask and quickly put on stopper -swirled flask in bath water until the pressure began to drop -plotted 8 points from the graph on lab quest (Pressure O2/time) -use this info to measure the slope -had 3 different trials where we kept the H2O2 constant on 2 of them and changed KI, and vice versa -the 4th trial we increased the temp and plotted 8 points |
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formula for slope/rate |
y2-y1/x2-x1 |
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if doubling either [H2O2] or [I] doubles the reaction what is the rate law? |
rate = k[H2O2][I] |
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what 6 factors may influence the rate of the reaction? |
1. nature of reactants 2. concentration of reactants 3. temperature 4. presence of a catalyst 5. order of reaction 6. energy |
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define the term catalyst |
a substance that changes the speed of a chemical reaction without undergoing a permanent chemical change in the process |
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what name is given to k in the rate law? |
specific rate constant |
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name one thing that a chemical equation tells you. |
what your reactants are what your catalyst is what your product is |
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name one thing that a chemical equation does not tell you |
the rate of the reaction |
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name two things that the rate depends on |
concentration of reactants temperature |
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before a reaction will occur, name two things reactants must do |
1. must collide 2. must have enough energy |
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name one thing the rate constant (k) in a rate law is dependent on. |
temperature |
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name one thing the rate constant (k) in a rate law is not dependent on. |
concentration |
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in the reaction we did in class what compound is disappearing? |
hydrogen peroxide (H2O2) |
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what compound are we measuring the appearance of? |
O2 |
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name the catalyst used for this reaction |
I- |
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what two experimental measurements do you need to calculate the order for each reactant? |
concentration time |
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how do you figure out the overall reaction from the rate law? |
add up the exponents |
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the energy barrier that must be overcome for a reaction to occur is called what? |
activation energy |
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what is chemical kinetics? |
the area of chemistry concerned with rates of chemical reactions
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rates of homogeneous reactions in solutions depend on ? |
1. nature of reactants 2. concentrations of reactants 3. temperature 4. presence of catalyst |
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what do catalyst do? |
they offer an alternate route to the reaction that requires less energy between reactant particles speeds up the reaction |
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what is the order of the reaction? |
the powers to which the concentration in the rate law are raised ex. rate=k[A]2 2nd order ex. rate=k[B] 1st order |
