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alexira [117]
3 years ago
6

Consider the following first-order reaction: A → B. The concentration of A at the start of the reaction is 4.17 M and after 4.84

s is 3.56 M. (a) Using the integrated rate law for a first-order reaction, calculate the value of the rate constant.
Chemistry
1 answer:
valina [46]3 years ago
4 0

Answer : The value of rate constant is, 0.0327s^{-1}

Explanation :

First we have to calculate the rate constant, we use the formula :

Expression for rate law for first order kinetics is given by:

k=\frac{2.303}{t}\log\frac{a}{a-x}

where,

k = rate constant  = ?

t = time passed by the sample  = 4.84 s

a = initial concentration = 4.17 M

a - x = concentration after time 4.84 s = 3.56 M

Now put all the given values in above equation, we get

k=\frac{2.303}{4.84}\log\frac{4.17}{3.56}

k=0.0327s^{-1}

Therefore, the value of rate constant is, 0.0327s^{-1}

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During endothermic phase change, the potential energy of the system always increases while the kinetic energy of the system remains constant. The potential energy of the reaction increases because energy is been added to the system from the external environment.

<u>Explanation</u>:

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Explanation:

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The gravitational potential energy of falling water is given by :

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Power is equal to the work done divided by time taken. So,

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