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In the reaction Mg+CuOarrow Cu+MgO the 'OXIDISING agent' is - -(1)... and the substance being OXIDISED is (2). 1: CuO;2:CuO 1:Mg;2:Mg 1:CuO;2:Mg 1:Mg;2:CuO

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In the reaction Mg+CuOarrow Cu+MgO the 'OXIDISING agent' is - -(1)... and the substance being OXIDISED is (2). 1: CuO;2:CuO 1:Mg;2:Mg 1:CuO;2:Mg 1:Mg;2:CuO

In the reaction Mg+CuOarrow Cu+MgO the 'OXIDISING agent' is - -(1)... and the substance being OXIDISED is (2). 1: CuO;2:CuO 1:Mg;2:Mg 1:CuO;2:Mg 1:Mg;2:CuO

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ErnestElite · Tutor for 8 years

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1: \( \mathrm{CuO} \); 2: \( \mathrm{Mg} \)

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## Step 1: Understanding the reaction<br />In the given reaction \( \mathrm{Mg}+\mathrm{CuO} \rightarrow \mathrm{Cu}+\mathrm{MgO} \), we can see that Magnesium (Mg) reacts with Copper Oxide (CuO) to produce Copper (Cu) and Magnesium Oxide (MgO).<br /><br />## Step 2: Identifying the oxidizing and reducing agents<br />In a redox (reduction-oxidation) reaction, the substance that is oxidized loses electrons, while the substance that is reduced gains electrons. The substance that causes another substance to be oxidized (by accepting its electrons) is the oxidizing agent, and the substance that causes another substance to be reduced (by giving away its electrons) is the reducing agent.<br /><br />In this reaction, Magnesium (Mg) is oxidized to Magnesium Oxide (MgO) as it loses electrons, and Copper Oxide (CuO) is reduced to Copper (Cu) as it gains electrons.<br /><br />### Therefore, the oxidizing agent is \( \mathrm{CuO} \) and the substance being oxidized is \( \mathrm{Mg} \).
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