Saved Bookmarks
| 1. |
The thermal decomposition of HCO_(2)H is a first order reaction with a rate constant of 2.4xx10^(-3)s^(-1) at a certain temmperature. Calculate how long will it take for three-fourths of initial quantity of HCO_(2)H to decompose. ""[log 0.25= -0.6021] |
|
Answer» Solution :Write the equation for the first order `t=(2.303)/(k)"LOG"([R]_(0))/(R )` When three-fourths of `HCO_(2)H` decomposes, the AMOUNT of `HCO_(2)H` that remains is one-fourth `i.e., R=([R]_(0))/(4)` Substituting the VALUES in the first order equation, we have `t=(2.303)/(2.4xx10^(-3)s^(-1)) "log"([R]_(0))/([R]_(0)//4)` `=(2.303)/(2.4xx10^(-3)s^(-1))log4` `=(2.303xx(0.6021))/(2.4xx10^(-3))=(2.303xx0.6021)/(2.4)xx10^(3)s` `=578` seconds. |
|