Multiple Choice
A compound consists of 36.33% carbon, 6.11% hydrogen, 21.20% nitrogen, and 36.31% oxygen. What is the empirical formula for this compound?
3. Chemical Reactions
Empirical Formula
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A hydrocarbon produced 0.0100 mol of carbon and 0.0150 mol of hydrogen during combustion. What is the empirical formula of the hydrocarbon?
A
C2H5
B
C2H3
C
CH2
D
CH
Verified step by step guidance1
Determine the moles of carbon and hydrogen given in the problem: 0.0100 mol of carbon and 0.0150 mol of hydrogen.
Find the simplest whole number ratio of moles of carbon to moles of hydrogen. Divide the moles of each element by the smallest number of moles present. In this case, divide both by 0.0100 mol.
Calculate the ratio: \( \frac{0.0100}{0.0100} = 1 \) for carbon and \( \frac{0.0150}{0.0100} = 1.5 \) for hydrogen.
Since the ratio for hydrogen is not a whole number, multiply both ratios by 2 to get whole numbers: 1 * 2 = 2 for carbon and 1.5 * 2 = 3 for hydrogen.
Write the empirical formula using the whole number ratios obtained: \( \text{C}_1\text{H}_3 \), which simplifies to \( \text{CH}_3 \).
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