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3 years ago

Which of the following is a nonmetal?a.iron b. silver c. oxygen d. copper

Chemistry

1 answer:

goldenfox [79]3 years ago

6 0

Oxygen because we couldn't use oxygen for the human body if it had metal in it.

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Storing sugar as long chains for later use is an example of a(n) ____________ chemical reaction.

DerKrebs [107]

Answer:

Endothermic

Explanation:

Storing sugar for later use is an example of an endothermic reaction because that energy is being absorbed.

8 0

3 years ago

Answer True or False for each of the following statements. (a) The carburization surface was maintained at slightly less than 0.

fomenos

Answer:

verdadero/a

falso/b

verdadero/c

Explanation:

6 0

2 years ago

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 ? H3

Margarita [4]

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

Explanation:

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:

Step 1: $H^++H_2O_2\rightleftharpoons H_3O_2^+;\text{ (fast)}$

Step 2: $H_3O_2^++Br^-\rightarrow HOBr+H_2O;\text{(slow)}$

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

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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2 years ago

In a certain variety of plants, red flowers appear in majority of plants and blue flowers appear only in a few plants. Which sta

Jlenok [28]

Answer:

Explanation:

3 0

3 years ago

Is gasoline a compound or a mixture? compound mixture

ehidna [41]

Gasoline would be a mixture if I recalled

3 0

3 years ago

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