Hydrogen iodide decomposes slowly to H2 and I2 at 600 K. The reaction is second order in HI, and the rate constant is 9.7×10−6M−1s−1. If the initial concentration of HI is 0.110 M. What is its molarity after a reaction time of 5.00 days? Express your answer in moles per liter to two significant figures.

Answer : The molarity after a reaction time of 5.00 days is, 0.109 M

Explanation :

The integrated rate law equation for second order reaction follows:

where,

k = rate constant =

t = time taken  = 5.00 days

[A] = concentration of substance after time 't' = ?

= Initial concentration = 0.110 M

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

Hence, the molarity after a reaction time of 5.00 days is, 0.109 M

petroleum? coal maybe?

in scientific notation, the value of the  speed of light in a vacuum

  will be written as 2.995 * 10^8. when this value is represented in the form of

  a * 10^b, then, a = 2.995 and b = 8.

the value of the speed of light in a vacuum given above can also be rounded up to approximately 300000000. in this case, the scientific notation will be written as 3 *10^8.