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Troyanec [42]
3 years ago
11

A particular reactant decomposes with a half-life of 113 s when its initial concentration is 0.372 M. The same reactant decompos

es with a half-life of 223 s when its initial concentration is 0.189 M. Calculate the rate constant (k) and reaction order?
Chemistry
1 answer:
AysviL [449]3 years ago
8 0

Answer:

Rate constant =  0.0237 M-1 s-1, Order = Second order

Explanation:

In this problem, it can be observed that as the concentration decreases, the half life increases. This means the concentration of the reactant is inversely proportional to the half life.

The order of reaction that exhibit this relationship is the second order of reaction.

In the second order of reaction, the relationship between rate constant and half life is given as;

t1/2 = 1 / k[A]o

Where;

k = rate constant

[A]o = Initial concentration

k = 1 / t1/2 [A]

Uisng the following values;

k = ?

t1/2 = 113

[A]o = 0.372M

k = 1 / (113)(0.372)

k = 1 / 42.036 = 0.0237 M-1 s-1

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2 years ago
The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O2 from the air
IceJOKER [234]

Answer:

1.75\cdot 10^{-4} M

Explanation:

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p^o = \chi_{O_2} p

Then the equation becomes:

S_1 = k_H \chi_{O_2} p

Solve for k_H:

k_H = \frac{S_1}{\chi_{O_2} p} = \frac{2.67\cdot 10^{-4} M}{0.209\cdot 1.00 atm} = 0.001278 M/atm

Now we're given that at an altitude of 12,000 ft, the atmospheric pressure is now:

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Apply Henry's law using the constant we found:

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3 years ago
For which process would the pictured cell be used?
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Answer:

Coating a material with metal

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1 year ago
How do you do this? very confused
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The problem you have written you almost have it solved.  Take the moles that you have calculated and multiply that by the molecular weight to get the grams.

The STP problem:
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From there you can solve for the volume

Hope this helps!
4 0
3 years ago
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