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Chapter 3: Problem 121

The greatest number of \(\mathrm{N}\) atoms is found in (a) \(50.0 \mathrm{g}\) \(\mathrm{N}_{2} \mathrm{O} ;\) (b) \(17.0 \mathrm{g} \mathrm{NH}_{3} ;\) (c) \(150 \mathrm{mL}\) of liquid pyridine, \(\mathrm{C}_{5} \mathrm{H}_{5} \mathrm{N}(d=0.983 \mathrm{g} / \mathrm{mL}) ;\) (d) \(1.0 \mathrm{mol} \mathrm{N}_{2}\)

Short Answer

Expert verified
After calculating and comparing the number of Nitrogen atoms for each substance, the substance with the largest number of Nitrogen atoms can be identified. Remember, always carry out these calculations carefully and thoughtfully.

Step by step solution

01

Calculate the number of moles for each compound

For each compound, use its molar mass and given mass or volume to find the number of moles. For \(N_2O\), use the molar mass approximately 44 g/mol, for \(NH_3\) use the molar mass about 17 g/mol. For Pyridine \(C_5H_5N\) first, we need to convert the volume to mass using the density (0.983 g/mL), then use molar mass which is approximately 79 g/mol. For \(N_2\), it's already in moles, so no further calculation is needed.
02

Calculate number of nitrogen atoms for each compound

For \(N_2O\), there are two nitrogen atoms, so double the number of moles. For \(NH_3\) there is one nitrogen atom, so the number of moles equals the number of Nitrogen atoms. For pyridine, there is one Nitrogen atom, so again, the number of moles equals the number of Nitrogen atoms. For \(N_2\), as there are 2 nitrogen atoms, double the number of moles.
03

Compare the final numbers

After calculating the number of Nitrogen atoms for each compound, compare these numbers to identify which is the largest and thus answer the original question.

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Most popular questions from this chapter

Determine the mass percent \(H\) in the hydrocarbon isooctane, \(\mathrm{C}\left(\mathrm{CH}_{3}\right)_{3} \mathrm{CH}_{2} \mathrm{CH}\left(\mathrm{CH}_{3}\right)_{2}\)

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