Chemistry, 03.07.2019 11:30 vlactawhalm29

When zinc metal reacts with oxygen gas, 2zn(s) + o2(g) → 2zno(g), large amounts of light and heat are released. a student states that this reaction is a combustion reaction but not a redox reaction. do you agree? defend your answer by explaining whether or not it meets the requirements of each type of reaction. asap

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Answer from: howto

The statement given by student is wrong because given reaction is an example of both redox reaction and combustion reaction.

Explanation:

1) A combustion reaction in general is defined as chemical reaction in which one substance reacts with oxygen gas along with release of heat.

$2Zn(s) + O_2(g)\rightarrow 2ZnO(g)$

Here Zn is reacting oxygen gas to give zinc oxide as a product along with release of heat.Yes,it is a combustion reaction

2) A redox reaction is defined as chemical reaction in which one substance from reactant undergoes oxidation and another substance from the reactants undergoes reduction reaction simultaneously.

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

$X^{n+}+ne^-\rightarrow X$

$2Zn(s) + O_2(g)\rightarrow 2ZnO(g)$

The given reaction an example of Redox reaction.

Here, in this given reaction zinc is oxidizing to zinc(II) ion and oxygen is getting reduced from its elemental form to oxide ion.Yes,it is also an example of redox reaction.

Answer from: Quest

1. o2(g)as a product

Answer from: Quest

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.