Answer:
The order of reaction is 2.
Rate constant is 0.0328 (M s)⁻¹
Explanation:
The rate of a reaction is inversely proportional to the time taken for the reaction.
As we are decreasing the concentration of the reactant the half life is increasing.
a) For zero order reaction: the half life is directly proportional to initial concentration of reactant
b) for first order reaction: the half life is independent of the initial concentration.
c) higher order reaction: The relation between half life and rate of reaction is:
Rate = ![\frac{1}{k[A_{0}]^{(n-1)}}](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7Bk%5BA_%7B0%7D%5D%5E%7B%28n-1%29%7D%7D)
Half life =![K\frac{1}{[A_{0}]^{(n-1)} }](https://tex.z-dn.net/?f=K%5Cfrac%7B1%7D%7B%5BA_%7B0%7D%5D%5E%7B%28n-1%29%7D%20%7D)
![\frac{(halflife_{1})}{(halflife_{2})}=\frac{[A_{2}]^{(n-1)}}{[A_{1}]^{(n-1)} }](https://tex.z-dn.net/?f=%5Cfrac%7B%28halflife_%7B1%7D%29%7D%7B%28halflife_%7B2%7D%29%7D%3D%5Cfrac%7B%5BA_%7B2%7D%5D%5E%7B%28n-1%29%7D%7D%7B%5BA_%7B1%7D%5D%5E%7B%28n-1%29%7D%20%7D)
where n = order of reaction
Putting values
![\frac{109}{231}=\frac{[0.132]^{(n-1)}}{[0.280]^{(n-1)}}](https://tex.z-dn.net/?f=%5Cfrac%7B109%7D%7B231%7D%3D%5Cfrac%7B%5B0.132%5D%5E%7B%28n-1%29%7D%7D%7B%5B0.280%5D%5E%7B%28n-1%29%7D%7D)
Hence n = 2
![halflife=\frac{1}{k[A_{0}]}](https://tex.z-dn.net/?f=halflife%3D%5Cfrac%7B1%7D%7Bk%5BA_%7B0%7D%5D%7D)
Putting values
K = 0.0328
Answer: ![Rate=k[L]^1[M]^2](https://tex.z-dn.net/?f=Rate%3Dk%5BL%5D%5E1%5BM%5D%5E2)
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.
![Rate=k[L]^x[M]^y](https://tex.z-dn.net/?f=Rate%3Dk%5BL%5D%5Ex%5BM%5D%5Ey)
(1)
k= rate constant
x = order with respect to L
y = order with respect to M
n =( x+y)= Total order
a) If [L] is doubled, the reaction rate will increase by a factor of 2:
![2\times Rate=k[2L]^x[M]^y](https://tex.z-dn.net/?f=2%5Ctimes%20Rate%3Dk%5B2L%5D%5Ex%5BM%5D%5Ey)
(2)
b) If [M] is doubled, the reaction rate will increase by a factor of 4:
![4\times Rate=k[L]^x[2M]^y](https://tex.z-dn.net/?f=4%5Ctimes%20Rate%3Dk%5BL%5D%5Ex%5B2M%5D%5Ey)
(3)
Dividing 2 by 1:
![\frac{2\times Rate}{Rate}=\frac{k[2L]^x[M]^y}{k[L]^x[M]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B2%5Ctimes%20Rate%7D%7BRate%7D%3D%5Cfrac%7Bk%5B2L%5D%5Ex%5BM%5D%5Ey%7D%7Bk%5BL%5D%5Ex%5BM%5D%5Ey%7D)
Dividing 3 by 1
![\frac{4\times Rate}{Rate}=\frac{k[L]^x[2M]^y}{k[L]^x[M]^y}](https://tex.z-dn.net/?f=%5Cfrac%7B4%5Ctimes%20Rate%7D%7BRate%7D%3D%5Cfrac%7Bk%5BL%5D%5Ex%5B2M%5D%5Ey%7D%7Bk%5BL%5D%5Ex%5BM%5D%5Ey%7D)
Thus rate law is: ![k[L]^1[M]^2](https://tex.z-dn.net/?f=k%5BL%5D%5E1%5BM%5D%5E2)
Answer:
A. Nuclear
Explanation:
This is because it could cause severe environmental damage in areas inhabited by the public
Please mark brainliest
Because they have the same number of valence electrons.
K ---> 38.7 g / 39.1 g/mol = 0.99
N ---> 13.9 g / 14.0 g/mol = 0.99
O ---> 47.4 g / 16.0 g/mol = 2.96
Divide by smallest:
K ---> 0.99 / 0.99 = 1
N ---> 0.99 / 0.99 = 1
O ---> 2.96 / 0.99 = 3
KNO3
