Q. What is the molar mass of \(\mathrm{CO_{2}}\)?

Q: What are the atomic masses of C and O to use?

Use standard atomic weights: m(C)\approx 12.01\ \text{g/mol}, m(O)\approx 16.00\ \text{g/mol}.

Q: Why is there a factor of 2 for oxygen in \mathrm{CO_2}?

Because the formula \mathrm{CO_2} has 2 oxygen atoms. Each contributes one m(O) to the total.

Q: What is the molar mass of \mathrm{CO_2} with rounded atomic masses?

Using C=12 and O=16: \[ M(\mathrm{CO_2})=12+2(16)=44\ \text{g/mol}. \]

Q: How would you compute the mass of a given amount, using molar mass?

Use m=n\times M. For example, m=(n\ \text{mol})(44.01\ \text{g/mol}).\]

Answer

To find the molar mass of carbon dioxide, add the atomic masses of its atoms.

Carbon: \(1 \text{ C} \times 12.01 = 12.01\)

Oxygen: \(2 \text{ O} \times 16.00 = 32.00\)

Total molar mass:

\[
12.01 + 32.00 = 44.01 \text{ g/mol}
\]

Final result: \(44.01 \text{ g/mol}\)

Detailed Explanation

The molar mass of carbon dioxide is found by adding the molar masses of its atoms: one carbon atom and two oxygen atoms.

Step 1: Identify the atoms in the formula

Carbon dioxide is \( \mathrm{CO_2} \), which contains:

\(1\) carbon atom
\(2\) oxygen atoms

Step 2: Write the atomic molar masses

Use standard atomic molar masses (in grams per mole):

Carbon: \( \mathrm{C} \approx 12.01\ \mathrm{g/mol} \)
Oxygen: \( \mathrm{O} \approx 16.00\ \mathrm{g/mol} \)

Step 3: Calculate the molar mass of \( \mathrm{CO_2} \)

The molar mass is:

\[
\mathrm{M}(\\mathrm{CO_2}) = 1(12.01) + 2(16.00)
\]

Step 4: Perform the arithmetic

\[
\mathrm{M}(\\mathrm{CO_2}) = 12.01 + 32.00 = 44.01\ \mathrm{g/mol}
\]

Final Answer

The molar mass of \( \mathrm{CO_2} \) is \( 44.01\ \mathrm{g/mol} \).

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General Chemistry FAQs

What are the atomic masses of \(C\) and \(O\) to use?

Use standard atomic weights: \(m(C)\approx 12.01\ \text{g/mol}\), \(m(O)\approx 16.00\ \text{g/mol}\).

How do you set up the molar mass calculation for \(\mathrm{CO_2}\)?

\[ M(\mathrm{CO_2})=1\cdot m(C)+2\cdot m(O).\]

What numerical value do you get for \(M(\mathrm{CO_2})\)?

\[ M(\mathrm{CO_2})=12.01+2(16.00)=44.01\ \text{g/mol}.\]

Why is there a factor of \(2\) for oxygen in \(\mathrm{CO_2}\)?

Because the formula \(\mathrm{CO_2}\) has \(2\) oxygen atoms. Each contributes one \(m(O)\) to the total.

What units should the molar mass be reported in?

\[ \text{grams per mole},\ \text{g/mol}. \]

What is the molar mass of \(\mathrm{CO_2}\) with rounded atomic masses?

Using \(C=12\) and \(O=16\): \[ M(\mathrm{CO_2})=12+2(16)=44\ \text{g/mol}. \]

How would you compute the mass of a given amount, using molar mass?

Use \(m=n\times M\). For example, \(m=(n\ \text{mol})(44.01\ \text{g/mol}).\]

What’s CO₂’s molar mass?
It’s about 44.01 g/mol.

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