Questions: What is the molar mass of this compound? C4H10 Remember to round to the hundredths place from the periodic table. 34.00 g / mol 32.00 g / mol 58.14 g / mol 485.20 g / mol

What is the molar mass of this compound?
C4H10
Remember to round to the hundredths place from the periodic table.
34.00 g / mol
32.00 g / mol
58.14 g / mol
485.20 g / mol

Transcript text: What is the molar mass of this compound? $\mathrm{C}_{4} \mathrm{H}_{10}$ Remember to round to the hundredths place from the periodic table. $34.00 \mathrm{~g} / \mathrm{mol}$ $32.00 \mathrm{~g} / \mathrm{mol}$ $58.14 \mathrm{~g} / \mathrm{mol}$ $485.20 \mathrm{~g} / \mathrm{mol}$

Solution

Solution Steps

Step 1: Identify the elements and their quantities in the compound

The compound given is $\mathrm{C}_{4} \mathrm{H}_{10}$. This means it contains 4 carbon (C) atoms and 10 hydrogen (H) atoms.

Step 2: Find the atomic masses of the elements

From the periodic table:

The atomic mass of carbon (C) is approximately 12.01 g/mol.
The atomic mass of hydrogen (H) is approximately 1.008 g/mol.

Step 3: Calculate the total mass of each element in the compound

For carbon: \(4 \times 12.01 \, \text{g/mol} = 48.04 \, \text{g/mol}\)
For hydrogen: \(10 \times 1.008 \, \text{g/mol} = 10.08 \, \text{g/mol}\)

Step 4: Sum the masses to find the molar mass of the compound

Add the total masses of carbon and hydrogen: \[ 48.04 \, \text{g/mol} + 10.08 \, \text{g/mol} = 58.12 \, \text{g/mol} \]

Final Answer

The molar mass of $\mathrm{C}_{4} \mathrm{H}_{10}$ is \(\boxed{58.12 \, \text{g/mol}}\).

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