Answer :

GinnyAnswer
To determine the molar mass of copper(II) nitrate, [tex]\( \text{Cu(NO}_3\text{)}_2 \)[/tex], we need to add the molar masses of all the atoms in the compound. Here are the steps:

1. Identify the atomic masses:
- Copper (Cu): [tex]\( 63.55 \, \text{g/mol} \)[/tex]
- Nitrogen (N): [tex]\( 14.01 \, \text{g/mol} \)[/tex]
- Oxygen (O): [tex]\( 16.00 \, \text{g/mol} \)[/tex]

2. Break down the formula and count the atoms:
- 1 atom of Copper (Cu)
- 2 atoms of Nitrogen (N), since we have two nitrate groups [tex]\( (NO_3) \)[/tex] and each contains one nitrogen atom
- 6 atoms of Oxygen (O), since each nitrate group [tex]\( (NO_3) \)[/tex] has 3 oxygen atoms and we have two nitrate groups

3. Calculate the contributions of each element:
- The mass contributed by Copper:
[tex]\[ 1 \times 63.55 \, \text{g/mol} = 63.55 \, \text{g/mol} \][/tex]
- The mass contributed by Nitrogen:
[tex]\[ 2 \times 14.01 \, \text{g/mol} = 28.02 \, \text{g/mol} \][/tex]
- The mass contributed by Oxygen:
[tex]\[ 6 \times 16.00 \, \text{g/mol} = 96.00 \, \text{g/mol} \][/tex]

4. Sum the total molar mass:
[tex]\[ 63.55 \, \text{g/mol} + 28.02 \, \text{g/mol} + 96.00 \, \text{g/mol} = 187.57 \, \text{g/mol} \][/tex]

Therefore, the molar mass of copper(II) nitrate, [tex]\( \text{Cu(NO}_3\text{)}_2 \)[/tex], is [tex]\( \boxed{187.57 \, \text{g/mol}} \)[/tex].

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