Multiple Choice
In an experiment, 10.0 g of sulfur and 10.0 g of oxygen react completely to form an oxide of sulfur. What is its empirical formula?
3. Chemical Reactions
Empirical Formula
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What mass (in g) of carbon is in a sample of acetone (CH3COCH3) that contains 6.02 x 10^23 atoms of hydrogen?
A
48 g
B
36 g
C
24 g
D
12 g
Verified step by step guidance1
First, identify the molecular formula of acetone, which is \( \text{CH}_3\text{COCH}_3 \). This indicates that one molecule of acetone contains 6 hydrogen atoms.
Next, determine the number of acetone molecules in the sample. Since there are \( 6.02 \times 10^{23} \) hydrogen atoms and each acetone molecule contains 6 hydrogen atoms, divide the number of hydrogen atoms by 6 to find the number of acetone molecules.
Calculate the number of carbon atoms in the sample. Each acetone molecule contains 3 carbon atoms, so multiply the number of acetone molecules by 3 to find the total number of carbon atoms.
Use Avogadro's number \( (6.02 \times 10^{23} \text{ atoms/mol}) \) to convert the number of carbon atoms to moles of carbon. Divide the total number of carbon atoms by Avogadro's number.
Finally, calculate the mass of carbon in grams. Multiply the moles of carbon by the molar mass of carbon \( (12.01 \text{ g/mol}) \) to find the mass of carbon in the sample.
2:26mWatch next
Master Empirical vs Molecular Formula with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Empirical Formula practice set
Problem sets built by lead tutorsExpert video explanations