Calculating the Empirical Formula of a Carbon-Hydrogen Compound with Google SEO Optimization

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When dealing with the analysis of chemical compounds, understanding how to determine their empirical formulas is a fundamental skill in chemistry. This article will guide you through the process using a specific example and provide SEO-optimized content to help your website rank better on Google.

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Introduction to the Problem

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A certain gas compound contains 82.8% carbon and 17.2% hydrogen by mass. The vapour density of this compound is 29. Our task is to find the empirical formula of the compound.

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Step-by-Step Methodology

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Let's break down the process of calculating the empirical formula into manageable steps:

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Step 1: Calculate the Moles of Each Element

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To begin, we assume the compound's mass as 100 grams. This simplifies the calculations. From this assumption:

" "" "Carbon (C): 82.8 grams" "Hydrogen (H): 17.2 grams" "" "

Now, we need to convert these grams into moles:

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Moles of Carbon 82.8 g / 12.01 g/mol ≈ 6.90 mol

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Moles of Hydrogen 17.2 g / 1.01 g/mol ≈ 17.03 mol

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Step 2: Find the Simplest Stoichiometric Ratio

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Next, we find the simplest whole-number ratio of moles by dividing both values by the smallest number of moles calculated:

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Moles of Carbon 6.90 mol / 6.90 mol 1

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Moles of Hydrogen 17.03 mol / 6.90 mol ≈ 2.47

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Step 3: Convert to Whole Numbers

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To convert the ratio to whole numbers, we can multiply both by 2 to simplify the ratio:

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Moles of Carbon 1 × 2 2

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Moles of Hydrogen 2.47 × 2 ≈ 5

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Step 4: Write the Empirical Formula

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Based on the calculations, the empirical formula of the compound is:

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CH5

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Step 5: Verify with Vapour Density

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To confirm our empirical formula is correct, we calculate the molar mass:

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Molar mass of CH5 (2 × 12.01) (5 × 1.008) 24.02 5.04 29.06 g/mol

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This matches the given vapour density of 29 g/mol, confirming our calculations.

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SEO-Optimized Content for Google

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Incorporating optimal keywords and H-tags can help your content rank higher on Google. Here’s how you might structure your SEO-optimized post:

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Calculating the Empirical Formula of a Carbon-Hydrogen Compound

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Learn how to calculate the empirical formula of a carbon-hydrogen compound with these step-by-step instructions. Understand the importance of using the given mass percentages, converting them to moles, and finding the simplest ratio.

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Understanding the Problem: Carbon and Hydrogen Percentages

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A compound is composed of 82.8% carbon and 17.2% hydrogen. We need to find the empirical formula of this compound, which is crucial for understanding its molecular structure.

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Critical Steps: Conversions and Calculations

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To find the empirical formula, we follow these essential steps:

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Step 1: Assumption and Conversion to Moles

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Assume the compound's mass is 100 grams, then convert the mass percentages to moles using the molar masses of carbon and hydrogen.

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Step 2: Ratio Calculation

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Determine the simplest whole-number ratio of moles by dividing by the smallest value.

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Step 3: Whole Number Conversion

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Convert the decimal values to whole numbers by multiplying by a suitable factor.

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Step 4: Determining the Empirical Formula

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Write down the empirical formula based on the simplified ratios.

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Verification with Vapour Density

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Verify the empirical formula using the given vapour density, which confirms the accuracy of the calculated molar mass.

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Understanding these steps and calculating the empirical formula can help solve similar problems in chemistry. Make sure to practice these calculations regularly to improve your problem-solving skills.

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Keywords: empirical formula, carbon-hydrogen compound, vapour density