Chemistry, 12.02.2020 03:12, vm204618

The half-reactions for the oxidation-reduction reaction between Al(s) and Zn₂ (aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s) if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients?

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answered: lordined5256

This is an incomplete question, here is a complete question.

$Al(s)\rightarrow Al^{3+}(aq)+3e^-$

$Zn^{2+}(aq)+2e^-\rightarrow Zn(s)$

The half-reactions for the oxidation-reduction reaction between Al(s) and Zn²⁺(aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s) if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients?

Answer : The coefficient for Al(s) is, 2

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

The given oxidation-reduction half reaction are :

Oxidation : $Al(s)\rightarrow Al^{3+}(aq)+3e^-$

Reduction : $Zn^{2+}(aq)+2e^-\rightarrow Zn(s)$

Now balance the charge.

In order to balance the electrons, we multiply the oxidation reaction by 2 and reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

Oxidation : $2Al(s)\rightarrow 2Al^{3+}(aq)+6e^-$

Reduction : $3Zn^{2+}(aq)+6e^-\rightarrow 3Zn(s)$

The balanced chemical equation will be,

$2Al(s)+3Zn^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Zn(s)$

Thus, the coefficient for Al(s) is, 2

answered: Guest

The answer is 323 g.

answered: Guest

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. $hbr$ completely dissociates to $h^+$ and $br-$ ions. a is incorrect because $h_2s$ does not fully ionize to $h^+$ and $hs^-$ ions and some remain as the compound $h_2s$ . c and d are incorrect because, $li_2o$ and $libr$ do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise, if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both $li_2o$ and $libr$ have a complete octet so can not accept any electrons which disqualifies them as acids.

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The half-reactions for the oxidation-reduction reaction between Al(s) and Zn₂ (aq) are represented a...