Question

Plzzz solve the problem​

Answer 1

$\bf{\odot \; UNBALANCED \; REACTION}$

$\sf \underset{Magnesium}{Mg\,(s)} \; + \; \underset{Oxygen}{O_2 \, (g)} \; \longrightarrow \; \underset{Magnesium \, Oxide}{MgO \, (s)}$

$\bf{\odot \; BALANCED \; REACTION}$

$\sf \underset{Magnesium}{2Mg\,(s)} \; + \; \underset{Oxygen}{O_2 \, (g)} \; \longrightarrow \; \underset{Magnesium \, Oxide}{2MgO \, (s)}$

• When magnesium ribbon is burnt in air, it combines with oxygen to form white powder magnesium oxide MgO with the release of heat and light. The reaction is exothermic in nature as a large amount of heat is released. Magnesium burns with dazzling white light so wear eyeglasses while performing this reaction and also rub the magnesium ribbon with sandpaper.

Answer 2

Answer:

When magnesium reacts with oxygen, the magnesium atoms donate electrons to O2 molecules and thereby reduce the oxygen. Magnesium therefore acts as a reducing agent in this reaction.

2 Mg + O2 ----> 2 MgO

reducing

agent

The O2 molecules, on the other hand, gain electrons from magnesium atoms and thereby oxidize the magnesium

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