Answer:
C. rate = k[F₂] [Cl₂O]
Explanation:
Based on the reaction, rate law can be obtained from the initial concentration of reactants thus:
rate = k[F₂]ᵃ [Cl₂O]ᵇ
Where the exponents a and b can be finded doing a experiment changing initial concentrations and seeing how a variation contribute in rate law.
If you analize experiments 1 and 2, the only change is [Cl₂O] (From 0.010 to 0.040, four times more) that changes its concentration in four times. This change produce rate law change from 5x10⁻⁴ to 2.0x10⁻³, also four times. That means the exponent b of [Cl₂O] is 1.
rate = k[F₂]ᵃ [Cl₂O]ᵇ
rate = k[F₂]ᵃ [Cl₂O]¹
Now, comparing experiments 1 and 3, the [F₂] change from 0.05 to 0.10, (Twice), and initial rate change from 5x10⁻⁴ to 1x10⁻³ (Also, twice). That means a = 1 and rate law is:
rate = k[F₂]¹ [Cl₂O]
rate = k[F₂] [Cl₂O]
Thus, right answer is:
<h3>C. rate = k[F₂] [Cl₂O]</h3>
Answer:
It sends an alarm to the building and saying there is a fire somewhere in the building.
Treat compound b with a strong base to get compounds C & D!
Answer:
It is an amorphous solid and hence also called pseudo solid. So it flows very slowly over thousands of years. It is not visible to the n*ked eye.
The moles of oxygen produced is calculated as follows
write a balanced reacting equation, that is
Mg(ClO3)2 ---->MgCl2 + 3O2
from the equation above the reacting ratio of Mg(ClO3)2 to O2 is 1: 3 therefore the moles of O2 produced = 5.12 moles x3 =15.36 moles