The decomposition reaction 2 hi(g) → h2(g) + 12(g), is second order and has a rate constant equal to 1.6 x 10m's at 700 °c. if the initial concentration of hi in the container is 3.4 x 10-m, how many minutes will it take for the concentration to be reduced to 8.0 x 104 m?

Answer : The time taken by the reaction is 12714.46 minutes.

Explanation :

The expression used for second order kinetics is:

where,

k = rate constant =

t = time = ?

= final concentration =

= initial concentration =

Now put all the given values in the above expression, we get:

     (1 min = 60 s)

Therefore, the time taken by the reaction is 12714.46 minutes.

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answer : one can design an experiment using a liquid and an additive that can be added to the liquid and observe the chemical changes in the reaction species.

one would need a beaker which is filled with a known amount of the liquid in which thermometer is placed to measure the temperature changes; after addition of the additive to the liquid solution one can note down the temperature change and find whether the reaction is endothermic or exothermic in nature. by subtracting the initial temperature value with the final temperature one can find the temperature changes.

various combinations of liquid and additive can be used. liquid in this case can be a known quantity of water and additives can be epsom salt or without epsom salt the experiment can be conducted to notice the changes. water and ice, hydrogen peroxide and dry yeast, vinegar and baking soda,etc.