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2 years ago

A compound with an empirical formula of CH3 has a molar mass of 60.2 g/mol. What is its molecular formula?

Chemistry

1 answer:

disa [49]2 years ago

5 0

Answer:

C₄H₁₂

Explanation:

The empirical formula gives you your smallest whole number ratio for the elements in the compound. Find the molar mass using a periodic table. We have one carbon (12.01 g/mol) and three hydrogens (1.008 g/mol). Therefore our molar mass for the empirical formula is 12.01 + 3(1.008) = 15.034 g/mol. To find the molecular formula divide the given molar mass by the empirical formula's molar mass 60.2/15.034 = 4.004257017 = 4. This number is the amount to multiply the empirical formula by to get the molecular formula, therefore your molecular formula is C₄H₁₂

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2 years ago

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3 years ago

Which conversion factor do you use first to calculate the number of grams of CO 2 produced by the reaction of 50.6 g of CH 4 wit

Brilliant_brown [7]

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The balanced chemical reaction is shown below:-

$CH_4+2O_2\rightarrow CO_2+2H_2O$

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Given, mass of methane = 50.6 g

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The formula for the calculation of moles is:-

$Moles=\frac{Mass\ taken}{Molar\ mass}=\frac{50.6}{16.04}\ mol=3.15\ mol$

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3 years ago