100 grams of magnesium and 2.50 grams of oxygen react together in synthesis reaction to form magnesium oxide. How do you write this balanced reaction?

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100 grams of magnesium and 2.50 grams of oxygen react together in synthesis reaction to form magnesium oxide. How do you write this balanced reaction?

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Answer 1 · 2016-04-30T15:27:46

The balanced equation is clearly:

$M g (s) + \frac{1}{2} O_{2} (g) \to M g O (s)$ $Mg(s) + 1/2O_2(g) rarr MgO(s)$

Explanation:

It is abundantly clear that magnesium is in vast molar excess:

i.e. $Moles of metal$ $"Moles of metal"$ $=$ $=$ $\frac{100 \cdot g}{24.31 \cdot g \cdot m o l^{- 1}}$ $(100*g)/(24.31*g*mol^-1)$ $≅$ $~=$ $5 \cdot m o l$ $5*mol$

$Moles of dioxygen$ $"Moles of dioxygen"$ $=$ $=$ $\frac{2.5 \cdot g}{32.00 \cdot g \cdot m o l^{- 1}}$ $(2.5*g)/(32.00*g*mol^-1)$ $≅$ $~=$ $0.08 \cdot m o l$ $0.08*mol$

Clearly, $O_{2}$ $O_2$ is the limiting reagent, and our calculation proceeds on the basis of the molar quantity of the gas.

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100 grams of magnesium and 2.50 grams of oxygen react together in synthesis reaction to form magnesium oxide. How do you write this balanced reaction?

1 Answer

Explanation:

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