Answer : The image is attached below.
Explanation :
For [tex]O_3[/tex]:
Molar mass, M = 48 g/mol
Mass, m = 24 g
Moles, n = [tex]\frac{m}{M}=\frac{24g}{48g/mol}=0.5mol[/tex]
Number of particles, N = [tex]n\times 6.022\times 10^{23}=0.5\times 6.022\times 10^{23}=3.0\times 10^{23}[/tex]
For [tex]NH_3[/tex]:
Molar mass, M = 17 g/mol
Mass, m = 170 g
Moles, n = [tex]\frac{m}{M}=\frac{170g}{17g/mol}=10mol[/tex]
Number of particles, N = [tex]n\times 6.022\times 10^{23}=10\times 6.022\times 10^{23}=6.0\times 10^{24}[/tex]
For [tex]F_2[/tex]:
Molar mass, M = 38 g/mol
Mass, m = 38 g
Moles, n = [tex]\frac{m}{M}=\frac{38g}{38g/mol}=1mol[/tex]
Number of particles, N = [tex]n\times 6.022\times 10^{23}=1\times 6.022\times 10^{23}=6.0\times 10^{23}[/tex]
For [tex]CO_2[/tex]:
Molar mass, M = 44 g/mol
Moles, n = 0.10 mol
Mass, m = [tex]n\times M=0.10mol\times 44g/mol=4.4g[/tex]
Number of particles, N = [tex]n\times 6.022\times 10^{23}=0.10\times 6.022\times 10^{23}=6.0\times 10^{22}[/tex]
For [tex]NO_2[/tex]:
Molar mass, M = 46 g/mol
Moles, n = 0.20 mol
Mass, m = [tex]n\times M=0.20mol\times 46g/mol=9.2g[/tex]
Number of particles, N = [tex]n\times 6.022\times 10^{23}=0.20\times 6.022\times 10^{23}=1.2\times 10^{23}[/tex]
For [tex]Ne[/tex]:
Molar mass, M = 20 g/mol
Number of particles = [tex]1.5\times 10^{23}[/tex]
Moles, n = [tex]\frac{N}{6.022\times 10^{23}}=\frac{1.5\times 10^{23}}{6.022\times 10^{23}}=0.25mol[/tex]
Mass, m = [tex]n\times M=0.25mol\times 20g/mol=5g[/tex]
For [tex]N_2O[/tex]:
Molar mass, M = 44 g/mol
Number of particles = [tex]1.2\times 10^{24}[/tex]
Moles, n = [tex]\frac{N}{6.022\times 10^{23}}=\frac{1.2\times 10^{24}}{6.022\times 10^{23}}=1.9mol[/tex]
Mass, m = [tex]n\times M=1.9mol\times 44g/mol=83.6g[/tex]
For unknown substance:
Number of particles = [tex]3.0\times 10^{23}[/tex]
Mass, m = 8.5 g
Moles, n = [tex]\frac{N}{6.022\times 10^{23}}=\frac{3.0\times 10^{23}}{6.022\times 10^{23}}=0.50mol[/tex]
Molar mass, M = [tex]\frac{m}{n}=\frac{8.5g}{0.50mol}=17g/mol[/tex]
The substance is [tex]NH_3[/tex].
