What is the molar mass of C4H10O?
Understand the Problem
The question is asking for the molar mass of the chemical compound with the formula C4H10O. To find the molar mass, we need to sum the atomic masses of all the atoms present in the compound, given that it contains 4 carbon (C) atoms, 10 hydrogen (H) atoms, and 1 oxygen (O) atom.
Answer
$74.12 \text{ g/mol}$
Answer for screen readers
The molar mass of the compound C$4$H${10}$O is $74.12 \text{ g/mol}$.
Steps to Solve
- Identify the atomic masses
We need to know the atomic masses of the elements in the compound. The atomic masses are approximately as follows:
- Carbon (C): 12.01 g/mol
- Hydrogen (H): 1.008 g/mol
- Oxygen (O): 16.00 g/mol
- Calculate total mass for each element
Next, we find the total mass contributed by each type of atom in the compound C$4$H${10}$O.
-
For Carbon (C): Total mass from carbon = number of carbon atoms × atomic mass of carbon [ \text{Mass from C} = 4 \text{ atoms} \times 12.01 \text{ g/mol} = 48.04 \text{ g/mol} ]
-
For Hydrogen (H): Total mass from hydrogen = number of hydrogen atoms × atomic mass of hydrogen [ \text{Mass from H} = 10 \text{ atoms} \times 1.008 \text{ g/mol} = 10.08 \text{ g/mol} ]
-
For Oxygen (O): Total mass from oxygen = number of oxygen atoms × atomic mass of oxygen [ \text{Mass from O} = 1 \text{ atom} \times 16.00 \text{ g/mol} = 16.00 \text{ g/mol} ]
- Sum the total masses
Now, we add all the total masses calculated in the previous step to find the molar mass of C$4$H${10}$O. [ \text{Molar Mass} = \text{Mass from C} + \text{Mass from H} + \text{Mass from O} ] [ \text{Molar Mass} = 48.04 \text{ g/mol} + 10.08 \text{ g/mol} + 16.00 \text{ g/mol} = 74.12 \text{ g/mol} ]
The molar mass of the compound C$4$H${10}$O is $74.12 \text{ g/mol}$.
More Information
The molar mass is important in chemistry as it allows for conversion between moles and grams, and is essential for stoichiometric calculations in reactions.
Tips
- Forgetting to multiply the atomic mass by the number of atoms for each element.
- Not summing all the total masses correctly.
- Misreading atomic masses from the periodic table.
