Multiple Choice
How many moles of atoms are in 5.00 g of ¹³C?
2. Atoms & Elements
Mole Concept
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The fuel used in many disposable lighters is liquid butane, C4H10. How many carbon atoms are in 1.50 g of butane given that the molar mass of butane is 58.12 g/mol? Express your answer numerically in atoms.
A
6.02 x 10^23 atoms
B
1.24 x 10^23 atoms
C
3.10 x 10^22 atoms
D
2.48 x 10^23 atoms
Verified step by step guidance1
Determine the number of moles of butane (C₄H₁₀) by using the formula: \( \text{moles of butane} = \frac{\text{mass of butane}}{\text{molar mass of butane}} \). Substitute the given values: mass = 1.50 g and molar mass = 58.12 g/mol.
Calculate the number of moles of butane using the values from the previous step.
Use Avogadro's number to find the total number of molecules of butane. Avogadro's number is \( 6.02 \times 10^{23} \) molecules/mol. Multiply the moles of butane by Avogadro's number.
Determine the number of carbon atoms in the butane molecules. Since each molecule of butane (C₄H₁₀) contains 4 carbon atoms, multiply the total number of butane molecules by 4.
Calculate the final number of carbon atoms using the result from the previous step.
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