Respuesta :
Answer: The molecular formula of the compound is [tex]NO_2[/tex]
Explanation:
Converting all these percentages into mass.
We take the total mass of the compound to be 100 grams, so, the percentages given for each element becomes its mass.So, the mass of each element is equal to the percentage given.
Mass of N = 30.45 g
Mass of O = 69.55 g
Step 1 : convert given masses into moles.
Moles of N=[tex]\frac{\text{ given mass of N}}{\text{ molar mass of N}}= \frac{30.45g}{14g/mole}=2.175moles[/tex]
Moles of O = [tex]\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{69.55g}{16g/mole}=4.347moles[/tex]
Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.
For N = [tex]\frac{2.175}{2.175}=1[/tex]
For O =[tex]\frac{4.347}{2.175}=2[/tex]
The ratio of N: O = 1: 2
Hence the empirical formula is [tex]NO_2[/tex].
Empirical mass of [tex]NO_2[/tex] is = 14(1)+16 (2)=46
The equation used to calculate the valency is:
[tex]n=\frac{\text{molecular mass}}{\text{empirical mass}}=\frac{46.01}{46}=1[/tex]
Step 3: To calculate the molecular formula=[tex]n\times {\text {Equivalent Formula}}=1\times NO_2=NO_2[/tex]
Hence, the molecular formula of the compound is [tex]NO_2[/tex]
1. The empirical formula for this compound is [tex]NO_2[/tex].
2. The molecular formula of the compound is [tex]NO_2[/tex].
Mass percentage:
So, the mass of each element is equal to the percentage given.
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Mass of N = 30.45 g
Mass of O = 69.55 g
Step 1 : Convert given masses into moles.
Moles of N= [tex]\frac{30.45g}{14g/mol} =2.175 moles[/tex]
Moles of O = [tex]\frac{69.55g}{16g/mol} =4.347 moles[/tex]
Step 2 : In order to get empirical formula, we will use mole-ratio concept.
For N = [tex]\frac{2.175}{2.175} =1[/tex]
For O = [tex]\frac{4.347}{2.175} =2[/tex]
The ratio of N : O = 1 : 2
Thus, the empirical formula is [tex]NO_2[/tex].
2. The molecular mass for this compound is [tex]NO_2[/tex].
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