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1. Identify the reducing agent in the following reactions.
\(2H_2\) + \(O_2\) → \(2H_2O\)
A reducing agent is an element that undergoes (becomes oxidised).
\(2H_2\) + \(O_2\) → \(2H_2O\)
In the above reaction, hydrogen \(2H_2\) is oxidized to water \(2H_2O\) by gaining an oxygen atom. Hence, hydrogen \(2H_2\) is a as it undergoes oxidation.
2. Identify the oxidising agent (oxidant) in the following reaction.
\(3Fe\) + \(4H_2O\) → \(Fe_3O_4\) + \(4H_2\)
An oxidising agent (oxidant) is a substance that another substance (by losing electrons or removing hydrogen or adding oxygen, or increasing oxidation state) while also being reduced.
\(3Fe\) + \(4H_2O\) → \(Fe_3O_4\) + \(4H_2\)
In the above reaction, water (\(H_2O\)) is the ; it oxidises iron (\(Fe\)) to form iron(III) oxide (\(Fe_3O_4\)) and hydrogen (\(H_2\)).
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