An organic compound contains 78% (by wt.) carbon and the remaining percentage of hydrogen. The right option for the empirical formula of this compound is : [Atomic wt. of C is 12, H is 1]
To find the empirical formula of the compound, we need to determine the simplest whole number ratio of carbon to hydrogen in the compound.
Determine the Mass of Carbon and Hydrogen: The compound contains 78% carbon by weight. Therefore, the percentage of hydrogen in the compound is: \(100\% - 78\% = 22\%\)
Calculate Moles of Each Element: For carbon, with an atomic weight of 12: \(\text{Moles of C} = \frac{78}{12} = 6.5\) For hydrogen, with an atomic weight of 1: \(\text{Moles of H} = \frac{22}{1} = 22\)
Determine the Simplest Whole Number Ratio: To find the simplest ratio, divide each by the smallest number of moles: \(\frac{6.5}{6.5} = 1 \quad \text{(for C)}\) \(\frac{22}{6.5} \approx 3.38\) Round \(3.38\) to the nearest whole number, which is 3.
Formulate the Empirical Formula: The empirical formula is determined as \(\text{CH}_3\).
Conclusion: The most simplified ratio of carbon to hydrogen in the compound is 1:3. Therefore, the empirical formula of the compound is \(\text{CH}_3\).
Organic Chemistry - Some Basic Principles and Techniques
Organic Chemistry is a subset of chemistry dealing with compounds of carbon. Therefore, we can say that Organic chemistry is the chemistry of carbon compounds and is 200-225 years old. Carbon forms bond with itself to form long chains of hydrocarbons, e.g.CH4, methane and CH3-CH3 ethane. Carbon has the ability to form carbon-carbon bonds quite elaborately. Polymers like polyethylene is a linear chain where hundreds of CH2 are linked together.
