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electrofy456
07.10.2020 •
Chemistry
Can some help me with this
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Ответ:
1.![Rate=k[CHCl_3]^1[Cl_2]^\frac{1}{2}](/tpl/images/0505/9699/bea07.png)
2. The rate constant (k) for the reaction is![3.50M^\frac{-1}{2}s^{-1}](/tpl/images/0505/9699/6eefe.png)
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
k= rate constant
x = order with respect to![CHCl_3](/tpl/images/0505/9699/a8390.png)
y = order with respect to![Cl_2](/tpl/images/0505/9699/cfbef.png)
n = x+y= Total order
1. a) From trial 1:
(1)
From trial 2:
(2)
Dividing 2 by 1 :![\frac{0.0069}{0.035}=\frac{k[0.020]^x[0.010]^y}{k[0.010]^x[0.010]^y}](/tpl/images/0505/9699/79be9.png)
b) From trial 2:
(3)
From trial 3:
(4)
Dividing 4 by 3:![\frac{0.0098}{0.0069}=\frac{k[0.020]^x[0.020]^y}{k[0.020]^x[0.010]^y}](/tpl/images/0505/9699/470b5.png)
2. to find rate constant using trial 1: