Answer:
[tex]0.0335\ \text{g}[/tex]
[tex]2.978\ \text{g}[/tex]
[tex]3586.84\ \text{g}[/tex]
[tex]0.0026\ \text{g}[/tex]
Explanation:
Mass in grams is given by
[tex]m=\dfrac{nM}{N_A}[/tex]
where
n = Number of molecules
[tex]N_A[/tex] = Avogadro's number = [tex]6.022\times 10^{23}\ \text{mol}^{-1}[/tex]
M = Molar mass of molecule
Molar mass of [tex]H_2O_2[/tex] = 34.0147 g/mol
[tex]n=5.94\times 10^{20}[/tex]
[tex]m=\dfrac{5.94\times 10^{20}\times 34.0147}{6.022\times 10^{23}}\\\Rightarrow m=0.0335\ \text{g}[/tex]
Mass of [tex]H_2O_2=0.0335\ \text{g}[/tex]
Molar mass of [tex]SO_2[/tex] = 64.066 g/mol
[tex]n=2.8\times 10^{22}[/tex]
[tex]m=\dfrac{2.8\times 10^{22}\times 64.066}{6.022\times 10^{23}}\\\Rightarrow m=2.978\ \text{g}[/tex]
Mass of [tex]SO_2=2.978\ \text{g}[/tex]
Molar mass of [tex]O_3[/tex] = 48 g/mol
[tex]n=4.5\times 10^{25}[/tex]
[tex]m=\dfrac{4.5\times 10^{25}\times 48}{6.022\times 10^{23}}\\\Rightarrow m=3586.84\ \text{g}[/tex]
Mass of [tex]O_3=3586.84\ \text{g}[/tex]
Molar mass of [tex]CH_4[/tex] = 16.04 g/mol
[tex]n= 9.85\times 10^{19}[/tex]
[tex]m=\dfrac{9.85\times 10^{19}\times 16.04}{6.022\times 10^{23}}\\\Rightarrow m=0.0026\ \text{g}[/tex]
Mass of [tex]CH_4=0.0026\ \text{g}[/tex]
