A compound has an empirical formula of $H C O_{2}$ $HCO_2$ and a molecular mass of 90 grams per mole. What is the molecular formula of this compound?

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A compound has an empirical formula of $H C O_{2}$ $HCO_2$ and a molecular mass of 90 grams per mole. What is the molecular formula of this compound?

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Answer 1 · 2016-02-25T16:07:09

The molecular formula is always a multiple of the empirical formula: ${(empirical formula)}_{n} = molecular formula$ $("empirical formula")_n ="molecular formula"$ .

Explanation:

So $(1.00794 + 12.011 + 2 \times 15.999) \cdot g \cdot m o l^{- 1} \times n$ $(1.00794 + 12.011 + 2xx15.999)*g*mol^-1xxn$ $=$ $=$ $90 \cdot g \cdot m o l^{- 1}$ $90*g*mol^-1$ .

We solve for $n$ $n$ , and clearly $n$ $n$ $=$ $=$ $2$ $2$ .

So empirical formula is $C_{2} H_{2} O_{4}$ $C_2H_2O_4$ .

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A compound has an empirical formula of $H C O_{2}$ $HCO_2$ and a molecular mass of 90 grams per mole. What is the molecular formula of this compound?

1 Answer

Explanation:

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A compound has an empirical formula of HCO_2HCO2HCO_2 and a molecular mass of 90 grams per mole. What is the molecular formula of this compound?

1 Answer

Explanation:

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A compound has an empirical formula of $H C O_{2}$ $HCO_2$ and a molecular mass of 90 grams per mole. What is the molecular formula of this compound?