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# What is the molecular formula for a compound that has an empirical formula of ${C_3}{H_7}$ and a molar mass of $86.2g/mol$?A. ${C_9}{H_{21}}$B. ${C_6}{H_{14}}$C. ${C_3}{H_7}$D. None of the above

Last updated date: 20th Jun 2024
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Hint: In chemistry, the empirical method of a chemical compound is the best superb integer ratio of atoms present in a compound. A simple instance of this idea is that the empirical formulation of sulfur monoxide, or $SO$, might virtually be $SO$, as is the empirical system of disulfur dioxide, ${S_2}{O_2}$.
Complete step by step solution:
Let the molecular formula of the compound is ${({C_3}{H_7})_n}$
Given molar mass of compound=
Molar mass of ${({C_3}{H_7})_n} = n(3 \times 12 + 7) = n(43)$
Then $n(43) = 86.2$
So $n = 2$
So, molecular formula is ${({C_3}{H_7})_2} = {C_6}{H_{14}}$

So the correct answer is B.

For organic compounds, carbon and hydrogen are listed as the first elements inside the molecular method, and they're accompanied by means of the remaining factors in alphabetical order. For instance, for butane, the molecular system is ${C_4}{H_{10}}$. For ionic compounds, the cation precedes the anion in the molecular system. For instance, the molecular method of sodium fluoride is $NaF$.