Which of the following is an example of redox reaction-?

Answer 1

A redox reaction (reduction and oxidation reaction) is a reaction in which there is a transfer of electrons. When an element is reduced, it gains electrons and its oxidation number is reduced. When an element is oxidized, it loses electrons and its oxidation number increases. Reduction and oxidation always happen at the same time.

There are seven rules to redox reactions and the formulas within them. # The oxidation number of a free element is zero (0). This includes Nitrogen (N2), Helium, Oxygen (O2), Ozone (O3) and S8. (Because there is no transfer of electrons, of course there would be no oxidation number!) # The oxidation number of a simple ion is its charge. For example, the oxidation number of Cl- is -1 and the oxidation number of Al3+ is +3. # The metals in Groups 1 and 2 (or 1A and 2A) have oxidation numbers of +1 and +2 respectively. # Hydrogen in combination usually has an oxidation number of +1. An exception to this rule are the metal hydrides (such as NaH), in which hydrogen has the oxidation number of -1. In other words, with Group 1 elements, Hydrogen will be -1. # Oxygen in combination usually has an oxidation number of -2. Exceptions to this rule include peroxide (such as H2O2, when Oxygen has to be -1) and oxygen-fluorine compounds, in which the oxidation number of oxygen is positive. This is because oxygen is the second-most electronegative element and usually takes electrons, but fluorine is the absolute most electronegative element and will take oxygen's electrons. # In a molecular or ionic compound, the sum of oxidation number totals must add to zero, since these compounds are electrically neutral. # In a polyatomic ion, the sum of the oxidation number totals must add to the charge of the ion.

With these rules in mind, we'll look at the formula in the synthesis of hydrogen and oxygen to make water.

2H2 + O2 => 2H20

Pure Hydrogen and pure Oxygen have an oxidation number of zero because of rule number 1.

In water, hydrogen has an oxidation number of +1 (rule 4) and oxygen would have an oxygen would have an oxidation number of -2 (rule 5). Hydrogen, therefore, is oxidized and oxygen is reduced.

Answer 2

An oxidator is oxidising a reductor by accepting electrons, in which reaction the oxidator is reduced by the reductor, :

So you see that everything is in vice verse, or in mirrored balance.

Example:

(1.) and (2.) together is the RED-OX = redox reaction (3.), note that electrons are to be equalised to get rid off)

1. O2 + 4 e- --> 2 O2- is the OXidator reaction
2. 2 H2 --> 4 H+ + 4 e- is the REDuctor reaction
3. O2 + 2 H2 + [4 e- ] --> [4 e- ] + [4 H+ + 2 O2- ] --> 2 H2O

Answer 3

Any equation that has a pure element on one side that is in a compound on the other side is a redox (reduction-oxidation) reaction because pure elements have an oxidation number of 0 and elements in compounds always have an oxidation number greater than or less than 0. There are literally millions of redox reactions.

2H2 + O2 = 2H2O

The Hydrogen and Oxygen on the left have oxidation numbers of 0 because they are pure. In water, Hydrogen has an oxidation number of 1+ and Oxygen has an oxidation number of 2-.

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Answer 4

The reaction between magnesium and oxygen to form magnesium oxide is an example of a redox reaction. In this reaction, magnesium undergoes oxidation by losing electrons to oxygen (reduction), while oxygen gains electrons from magnesium (oxidation).

Answer 5

2 Na +2 H2O ->2 NaOH + H2

In the above example, sodium (Na) gets oxidized while hydrogen gets reduced.

Answer 6

2Al + Mg(SO4) -> Mg + Al2(SO4)3

In this reaction, Al undergoes oxidation because its charge increases from 0 to +3. Mg undergoes reduction because its charge decreases from +2 to 0.

Answer 7

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Answer 8

Redox reaction is chemical reactions. This happens when atoms oxidation state changes.

Answer 9

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