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Montano1993 [528]
3 years ago
10

A reaction takes place between an acid and 0.5 gram of solid magnesium ribbon. Another reaction takes place between an acid and

0.5 grams of powdered magnesium which statement is true?
A.The powdered magnesium reacts faster because it has a greater surface area

B. The powdered magnesium reacts faster because the activation energy has been lowered

C.The magnesium strip reacts faster because it has a higher concentration of magnesium

D. The magnesium strip reacts faster because it will create a higher temperature once the reaction starts
Chemistry
1 answer:
aliina [53]3 years ago
5 0

Answer:

A

Explanation:

The correct answer would be that <u>the powdered magnesium reacts faster because it has a greater surface area</u>.

<em>The rate of reaction is defined as the rate of disappearance of the reactants in a reaction or the rate of conversion of appearance of products during a reaction. </em>

The rate of reaction is dependent on several factors such as the concentration of the reactants, temperature of the reaction, nature of reactants, and the presence or absence of catalysts during the reaction.

As far as the nature of reactants is concerned, the surface area of reactants comes into play. <em>Reactants with higher surface areas react faster than reactants with lesser surface areas</em>. Hence, powdery reactants react faster than solid reactants because the latter has a higher surface area than the former.

The correct option is A.

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Which of Hubble's findings supported the big bang theory? Check all that apply.
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<u>Out of all given options, Hubble's findings supported the big bang theory are as follows: </u>

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Option C, D, and E

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A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.18 M solution of H₂A?
Tcecarenko [31]

Answer:

pH = 2.10

Explanation:

We name an acid as diprotic because it can release two protons:

H₂A  +  H₂O  ⇄  H₃O⁺   + HA⁻     Ka₁

HA⁻  +  H₂O  ⇄  H₃O⁺   + A⁻²      Ka₂

We propose the mass balance:

Analytical concentration = [H₂A] +  [HA⁻]  + [A⁻²]

As Ka₂ is so small, we avoid the [A⁻²] so:

0.18 M = [H₂A] +  [HA⁻]

But we can not avoid the HA⁻, because the Ka₁. Ka₁'s expression is:

Ka₁ = [H₃O⁺] . [HA⁻] / [H₂A]

We propose the charge balance:

[H₃O⁺] = [HA⁻] + [A⁻²] + [OH⁻]

As we did not consider the A⁻², we can miss the term and if

Kw = H⁺ . OH⁻

We replace Kw/H⁺ = OH⁻. So the new equation is:

[H₃O⁺] = [HA⁻] + Kw / [H₃O⁺]

The acid is so concentrated, so we can avoid the term with the Kw, so:

[H₃O⁺] = [HA⁻]

In the mass balance we would have:

0.18 M = [H₂A]

We replace at Ka₁

Ka₁ = [H₃O⁺] . [HA⁻] / [H₂A]

Ka1 . 0.18 / [H₃O⁺] = [HA⁻]

We replace at the charge balance:

[H₃O⁺] = Ka1 . 0.18 / [H₃O⁺]

[H₃O⁺]² = 3.4×10⁻⁴  . 0.18

[H₃O⁺] = √(3.4×10⁻⁴  . 0.18)

[H₃O⁺] = 7.82×10⁻³

- log [H₃O⁺] = pH → - log 7.82×10⁻³

pH = 2.10

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