D as the two substances could have close boiling points, so if the temperature is not controlled well, both substances will evaporate.
In general, we have this rate law express.:
![\mathrm{Rate} = k \cdot [A]^x [B]^y](https://tex.z-dn.net/?f=%5Cmathrm%7BRate%7D%20%3D%20k%20%5Ccdot%20%5BA%5D%5Ex%20%5BB%5D%5Ey)
we need to find x and y
ignore the given overall chemical reaction equation as we only preduct rate law from mechanism (not given to us).
then we go to compare two experiments in which only one concentration is changed
compare experiments 1 and 4 to find the effect of changing [B]
divide the larger [B] (experiment 4) by the smaller [B] (experiment 1) and call it Δ[B]
Δ[B]= 0.3 / 0.1 = 3
now divide experiment 4 by experient 1 for the given reaction rates, calling it ΔRate:
ΔRate = 1.7 × 10⁻⁵ / 5.5 × 10⁻⁶ = 34/11 = 3.090909...
solve for y in the equation
![\Delta \mathrm{Rate} = \Delta [B]^y](https://tex.z-dn.net/?f=%5CDelta%20%5Cmathrm%7BRate%7D%20%3D%20%5CDelta%20%5BB%5D%5Ey)

To this point,
![\mathrm{Rate} = k \cdot [A]^x [B]^1](https://tex.z-dn.net/?f=%5Cmathrm%7BRate%7D%20%3D%20k%20%5Ccdot%20%5BA%5D%5Ex%20%5BB%5D%5E1%20)
do the same to find x.
choose two experiments in which only the concentration of B is unchanged:
Dividing experiment 3 by experiment 2:
Δ[A] = 0.4 / 0.2 = 2
ΔRate = 8.8 × 10⁻⁵ / 2.2 × 10⁻⁵ = 4
solve for x for
![\Delta \mathrm{Rate} = \Delta [A]^x](https://tex.z-dn.net/?f=%5CDelta%20%5Cmathrm%7BRate%7D%20%3D%20%5CDelta%20%5BA%5D%5Ex)

the rate law is
Rate = k·[A]²[B]
I’m not sure but I think the answer is substance . Because you can change the temperate of a substance but it will still be that substance . You can change all of these things except the substance itself
The mole ratio Aluminium to Aluminum Oxide is 2 : 1
<h3>Further explanation</h3>
Given
Reaction
2Al + Fe ----> Al2O3 +2Fe
Required
The mol ratio
Solution
If we look at the reaction above, there is an element missing from the reactant i.e oxygen, because the number of atoms and elements involved in the reaction should be the same between the reactants and products.
So the possible and balanced reactions are:
<em>2Al(s) + Fe₂O₃ (s) → Al₂O₃ (s)+ 2Fe (s) </em>
From this reaction the ratio of Al: Al₂O₃ can be determined, which is 2: 1
Answer:
Ksp = 0.0036.
Explanation:
Hello there!
In this case, according to the given information, it turns out possible for us to calculate the Ksp of the silver acetate, by knowing that its equilibrium expression is:
![Ksp=[Ag^+][CH_3COO^-]](https://tex.z-dn.net/?f=Ksp%3D%5BAg%5E%2B%5D%5BCH_3COO%5E-%5D)
Next, we calculate molar concentration of the ions in the solution, the same to that of the acetate ions, due to the 1:1 mole ratio, as follows:
![[Ag^+]=[CH_3COO^-]=\frac{1.0g/(166.9122 g/mol)}{0.1000L} =0.0600M](https://tex.z-dn.net/?f=%5BAg%5E%2B%5D%3D%5BCH_3COO%5E-%5D%3D%5Cfrac%7B1.0g%2F%28166.9122%20g%2Fmol%29%7D%7B0.1000L%7D%20%3D0.0600M)
Therefore, the Ksp is:

Regards!