QQuestionChemistry
QuestionChemistry
# Question 1
What is the molar mass of $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$ in $\mathrm{g} / \mathrm{mol}$ ? Click here for a copy of the periodic table.
- $149.10 \mathrm{~g} / \mathrm{mol}$
- $113.01 \mathrm{~g} / \mathrm{mol}$
- $141.03 \mathrm{~g} / \mathrm{mol}$
- $61.99 \mathrm{~g} / \mathrm{mol}$
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Answer
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Step 1:: Identify the molar masses of each element in the compound.
The chemical formula for the compound is $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$.
To find the molar mass, we need to find the molar mass of each element and then add them together. From the periodic table, we find: - Nitrogen (N): 14.01 g/mol - Hydrogen (H): 1.01 g/mol - Phosphorus (P): 30.97 g/mol - Oxygen (O): 16.00 g/mol
Step 2:: Calculate the molar mass of each group in the compound.
Molar mass of $\mathrm{NH}_{4}^{+}$ = Molar mass of N + (4 × Molar mass of H)
= 14.01 g/mol + (4 × 1.01 g/mol) = 14.01 g/mol + 4.04 g/mol = 18.05 g/mol
Step 3:: Calculate the molar mass of the compound.
Molar mass of $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$ = (3 × Molar mass of $\mathrm{NH}_{4}^{+}$) + Molar mass of P + (4 × Molar mass of O)
= (3 × 18.05 g/mol) + 30.97 g/mol + (4 × 16.00 g/mol) = 54.15 g/mol + 30.97 g/mol + 64.00 g/mol = 149.12 g/mol
Step 4:: Compare the calculated molar mass with the given options.
The calculated molar mass of $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$ is 149.12 g/mol, which is closest to the option 149.10 g/mol.
Final Answer
The molar mass of $\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}$ is approximately 149.10 g/mol.
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