Q. Molar mass of \( \mathrm{NH_3} \).

Q: What is the molar mass of ammonia, \mathrm{NH_3} ?

M = 14.01 + 3(1.008) \approx 17.03\ \mathrm{g/mol} .

Q: What atomic masses should be used to find M(\mathrm{NH_3}) ?

Use standard atomic masses: \mathrm{N} \approx 14.01\ \mathrm{g/mol} and \mathrm{H} \approx 1.008\ \mathrm{g/mol} .

Q: How do you set up the molar mass calculation for \mathrm{NH_3} ?

M(\mathrm{NH_3}) = 1(14.01) + 3(1.008) . Add nitrogen’s mass plus three times hydrogen’s mass.

Q: What is the molar mass of \mathrm{NH_3} using rounded atomic weights?

Using \mathrm{N}=14.0 and \mathrm{H}=1.0 : M = 14.0 + 3(1.0) = 17.0\ \mathrm{g/mol} .

Q: Is the molar mass in grams per mole or grams per molecule?

Molar mass is \mathrm{g/mol} for the entire formula unit (one mole of \mathrm{NH_3} molecules).

Q: How many grams of \mathrm{NH_3} correspond to 1 mole?

By definition, 1\ \text{mol}\ \mathrm{NH_3} has mass equal to M(\mathrm{NH_3}) \approx 17.03\ \mathrm{g} .

Answer

To find the molar mass of ammonia \( \mathrm{NH_3} \), add the atomic masses of \(1\) nitrogen and \(3\) hydrogens.

\[
M(\mathrm{NH_3}) = 1 \cdot M(\mathrm{N}) + 3 \cdot M(\mathrm{H})
\]

Using \(M(\mathrm{N}) \approx 14.01\ \mathrm{g/mol}\) and \(M(\mathrm{H}) \approx 1.008\ \mathrm{g/mol}\):

\[
M(\mathrm{NH_3}) = 14.01 + 3(1.008) = 17.034 \approx 17.03\ \mathrm{g/mol}
\]

Final result: \(17.03\ \mathrm{g/mol}\)

Detailed Explanation

To find the molar mass of ammonia, \(\mathrm{NH_3}\), you add the atomic masses of all atoms in one molecule.

Step 1: Identify the atoms in \(\mathrm{NH_3}\)

\(\mathrm{NH_3}\) contains:

\(\,1\) nitrogen atom (\(\mathrm{N}\)) and \(\,3\) hydrogen atoms (\(\mathrm{H}\)).

Step 2: Use standard atomic masses

Use these common periodic table values (in \(\mathrm{g/mol}\)):

\(\mathrm{N} \approx 14.01\ \mathrm{g/mol}\)

\(\mathrm{H} \approx 1.008\ \mathrm{g/mol}\)

Step 3: Multiply by the number of each atom

Nitrogen contribution:

\[
14.01\ \mathrm{g/mol}
\]

Hydrogen contribution (there are 3 hydrogens):

\[
3 \times 1.008\ \mathrm{g/mol} = 3.024\ \mathrm{g/mol}
\]

Step 4: Add them to get the molar mass

\[
\text{Molar mass of } \mathrm{NH_3} = 14.01 + 3.024 = 17.034\ \mathrm{g/mol}
\]

Final Answer

The molar mass of \(\mathrm{NH_3}\) is \(\boxed{17.03\ \mathrm{g/mol}}\) (rounded to two decimal places).

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General Chemistry FAQs

What is the molar mass of ammonia, \( \mathrm{NH_3} \)?

\( M = 14.01 + 3(1.008) \approx 17.03\ \mathrm{g/mol} \).

What atomic masses should be used to find \( M(\mathrm{NH_3}) \)?

Use standard atomic masses: \( \mathrm{N} \approx 14.01\ \mathrm{g/mol} \) and \( \mathrm{H} \approx 1.008\ \mathrm{g/mol} \).

How do you set up the molar mass calculation for \( \mathrm{NH_3} \)?

\( M(\mathrm{NH_3}) = 1(14.01) + 3(1.008) \). Add nitrogen’s mass plus three times hydrogen’s mass.

What is the molar mass of \( \mathrm{NH_3} \) using rounded atomic weights?

Using \( \mathrm{N}=14.0 \) and \( \mathrm{H}=1.0 \): \( M = 14.0 + 3(1.0) = 17.0\ \mathrm{g/mol} \).

Is the molar mass in grams per mole or grams per molecule?

Molar mass is \( \mathrm{g/mol} \) for the entire formula unit (one mole of \( \mathrm{NH_3} \) molecules).

How many grams of \( \mathrm{NH_3} \) correspond to 1 mole?

By definition, \( 1\ \text{mol}\ \mathrm{NH_3} \) has mass equal to \( M(\mathrm{NH_3}) \approx 17.03\ \mathrm{g} \).

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