Q. \( \text{molar mass of mg} \)

Q: How do I find molar mass if I know the chemical formula?

Add atomic masses: M=\sum n_i \times (\text{atomic mass of element } i). Use the periodic table, multiply each element’s atomic mass by its subscript, then sum.

Q: If I have mass in mg, how do I convert to moles?

Convert mg to g: m(\text{g})=m(\text{mg})/1000. Then n=m/M, with M in g/mol. So n=\frac{m(\text{mg})/1000}{M}.

Q: What is the relationship between moles, molar mass, and grams?

n=\frac{m}{M}, m=nM, and M=\frac{m}{n}. Units must match: m in g, M in g/mol, n in mol.

Q: How do I compute molar mass for a compound like \text{H}_2\text{SO}_4?

M=2(\text{H})+1(\text{S})+4(\text{O}). Plug in atomic masses (e.g., H \approx 1.008, S \approx 32.06, O \approx 16.00) and sum.

Answer

If the problem means magnesium, \(\text{Mg}\):

\[
\text{Molar mass of }\text{Mg} = 24.31\ \text{g mol}^{-1}
\]

Final result: \(\boxed{24.31\ \text{g mol}^{-1}}\)

Detailed Explanation

Step 1: Identify the element.

The chemical formula for magnesium is \( \mathrm{Mg} \).

Step 2: Use the periodic table atomic mass.

The standard atomic (molar) mass of magnesium is approximately:

\[
\mathrm{Mg}: \; 24.305 \ \mathrm{g\ mol^{-1}}
\]

Step 3: State the molar mass with correct units.

Molar mass is reported in grams per mole. Therefore, the molar mass of magnesium is:

\[
\boxed{24.305 \ \mathrm{g\ mol^{-1}}}
\]

Final answer.

\[
\boxed{24.305 \ \mathrm{g\ mol^{-1}}}
\]

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General Chemistry FAQs

What is “molar mass of \(\text{mg}\)” actually asking?

It likely means molar mass of a given compound, but “mg” is a unit of mass (milligrams), not a substance. You must know the compound or its chemical formula.

How do I find molar mass if I know the chemical formula?

Add atomic masses: \(M=\sum n_i \times (\text{atomic mass of element } i)\). Use the periodic table, multiply each element’s atomic mass by its subscript, then sum.

If I have mass in mg, how do I convert to moles?

Convert mg to g: \(m(\text{g})=m(\text{mg})/1000\). Then \(n=m/M\), with \(M\) in g/mol. So \(n=\frac{m(\text{mg})/1000}{M}\).

What is the relationship between moles, molar mass, and grams?

\(n=\frac{m}{M}\), \(m=nM\), and \(M=\frac{m}{n}\). Units must match: \(m\) in g, \(M\) in g/mol, \(n\) in mol.

Why can’t molar mass be given in mg/mol?

Molar mass is an intensive property typically reported in g/mol. mg/mol is equivalent numerically to g/mol divided or multiplied by \(1000\), but standard convention is g/mol.

How do I compute molar mass for a compound like \(\text{H}_2\text{SO}_4\)?

\(M=2(\text{H})+1(\text{S})+4(\text{O})\). Plug in atomic masses (e.g., H \(\approx 1.008\), S \(\approx 32.06\), O \(\approx 16.00\)) and sum.

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