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Kamila [148]
3 years ago
5

PLZ ANSWER

Chemistry
1 answer:
satela [25.4K]3 years ago
7 0

Answer:

B. The student should model a convex lens because it directs light toward the center of the lens.

Explanation:

Lenses are optical devices that work on the principle of refraction.

Refraction is a phenomenon of wave (such as light waves) that occurs when a ray of light crosses the interface between two mediums with different optical density: when this occurs, the ray of light bends and change speed.

In particular, there are two types of lenses:

  • Convex lenses: these lenses are curved outward at their center, therefore the rays of light coming from infinite distance (parallel to the axis) are all focused into a point of the lens, called principal focus. Therefore, a convex lens directs lights towards this point.
  • Concave lenses: these lenses are curved inward at their center, therefore the rays of light coming from infinite distance are bent away from the principal focus. Therefore, this is a diverging lens, as the rays of light do not converge.

So, the correct answer is

B. The student should model a convex lens because it directs light toward the center of the lens.

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<u>Answer:</u> The rate law for the reaction is \text{Rate}=k'[H+][H_2O_2][Br^-]

<u>Explanation:</u>

Rate law is the expression which is used to express the rate of the reaction in terms of the molar concentration of reactants where each term is raised to the power their stoichiometric coefficient respectively from a balanced chemical equation.

In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.

The chemical equation for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution follows:

2H^++2Br^-+H_2O_2\rightarrow Br_2+2H_2O

The intermediate reaction of the mechanism follows:

<u>Step 1:</u>  H^++H_2O_2\rightleftharpoons H_3O_2^+;\text{ (fast)}

<u>Step 2:</u>  H_3O_2^++Br^-\rightarrow HOBr+H_2O;\text{(slow)}

<u>Step 3:</u>  HOBr+H^++Br^-\rightarrow Br_2+H_2O;\text{(fast)}

As, step 2 is the slow step. It is the rate determining step

Rate law for the reaction follows:

\text{Rate}=k[H_3O_2^+][Br^-]          ......(1)

As, [H_3O_2^+] is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.

Applying steady state approximation for [H_3O_2^+] from step 1, we get:

K=\frac{[H_3O_2^+]}{[H^+][H_2O_2]}  

[H_3O_2^+]=K[H^+][H_2O_2]

Putting the value of [H_3O_2^+] in equation 1, we get:

\text{Rate}=k.K[H^+][H_2O_2][Br^-]\\\\\text{Rate}=k'[H+][H_2O_2][Br^-]

Hence, the rate law for the reaction is \text{Rate}=k'[H+][H_2O_2][Br^-]

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