Answer:
Explanation:
Hello,
In this case, we first apply the ideal gas equation to compute the moles of produced chlorine:
Then, by considering the given reaction, applying the stoichiometry, that shows a 1 to 1 relationship between chlorine and manganese dioxide, we find:
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Explanation:
here's the answer to your question
Explanation:
Half life is the amount of time taken by a radioactive material to decay to half of its original value.
Half life for second order kinetics is given by:
k = rate constant =?
= initial concentration
a = concentration left after time t
Integrated rate law for second order kinetics is given by:
a) Initial concentration of XY =
Rate constant of the reaction = k =
Half life of the reaction is:
1,436.78 seconds is the half-life for this reaction.
b) Initial concentration of XY = 0.100 M
Final concentration after time t = 12.5% of 0.100 M = 0.0125 M
Solving for t;
t = 10,057.47 seconds
In 10,057.47 seconds the concentration of XY will become 12.5% of its initial concentration.
c) Initial concentration of XY = 0.200 M
Final concentration after time t = 12.5% of 0.200 M = 0.025 M
Solving for t;
t = 5,028.73 seconds
In 5,028.73 seconds the concentration of XY will become 12.5% of its initial concentration.
d) Initial concentration of XY = 0.160 M
Final concentration after time t =
Solving for t;
t = 1,419.40 seconds
In 1,419.40 seconds the concentration of XY will become .
e) Initial concentration of
Final concentration after time t = x
t = 55.0 s
Solving for x;
x = 0.04906 M
The concentration after 55.0 seconds is 0.04906 M.
f) Initial concentration of XY= 0.050 M
Final concentration after time t = x
t = 500 s
Solving for x;
x = 0.04259 M
The concentration after 500 seconds is 0.0.04259 M.