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Preparations and Reactions of Sodium Oxide

If 0.1 g atom...

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If 0.1 g atom of magnesium is allowed to react with 2g molecule of oxygen then which of the following is correct for given equation? 2Mg (s) + O2 (g) = 2MgO (s) 1 )oxygen is the limiting reagent 2) magnesium is the limiting reagent 3 )0.02 moles of magnesium oxide is formed 4 )0.5 moles of oxygen remains in excess

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2 M g + O_{2} \to 2 M g O

Use the equation above to answer the following question.
If

0.486 g

of magnesium and

6.022 \times 10^{20}

molecules of oxygen react, what mass of magnesium oxide will be formed?

2 M g + O_{2} \to 2 M g O

, Calculate how much oxygen (in grams) required to combust

10

moles of Magnesium from the given equation.

2 Mg (s) + O_{2} (g) \to 2 MgO (s)

In the given equation, magnesium (Mg) is a .

2 M g (s) + O_{2} (g) \to 2 M g O (s)

0.243 g

of magnesium is fully oxidized, what volume of oxygen will be used up? Assume STP conditions.

Q. The mass of magnesium oxide formed by burning

1.216 g

magnesium in excess oxygen is:

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Preparations and Reactions of Sodium Oxide

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