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How many grams of nitrogen are contained in a sample of C4H9N3O2 that also contains 9.42x10^24 hydrogen atoms?

User Dave Wanta
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1 Answer

6 votes

Answer:

73.02 grams

Explanations:

Given the following parameter

Atom of hydrogen = 9.42x10^24 atoms

From the given compound, for every 9 moles of hydrogen, there are 3 moles of nitrogen, hence the atoms of nitrogen present in the compound will be:


\begin{gathered} atoms\text{ of nitrogen}=(3)/(9)*9.42*10^(24) \\ atoms\text{ of nitrogen}=3.14*10^(24)atoms \end{gathered}

Convert atoms to moles


\begin{gathered} moles\text{ of nitrogen}=(3.14*10^(24))/(6.02*10^(23)) \\ moles\text{ of nitrogen}=0.521*10 \\ moles\text{ of nitrogen}=5.21moles \end{gathered}

Convert moles of nitrogen to mass


\begin{gathered} mass\text{ of nitrogen}=mole* molar\text{ mass} \\ mass\text{ of nitrogen}=5.21moles*(14g)/(mol) \\ mass\text{ of nitrogen}=73.02grams \end{gathered}

Hence the mass of nitrogen contained in the sample is 73.02 grams

User Bemug
by
8.4k points
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