Phosphorus forms two oxides, which have the empirical formulae ${\mathrm{P}}_2{\mathrm{O}}_3$ and ${\mathrm{P}}_2{\mathrm{O}}_5$. Suggest the molecular formula for the oxides.? $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{P}=31, \mathrm{O}= 16\right]$

Zinc and phosphorus react to give zinc phosphide. $9.75 \mathrm{g}$ of zinc combines with $3.1 \mathrm{g}$ of phosphorus. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Zn}=65, \mathrm{P}=31\right]$

Find the empirical formula for the compound.

Calculate the percentage of phosphorus in it.

$110 \mathrm{g}$ of manganese was extracted from $174 \mathrm{g}$ of manganese oxide. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Mn}=55, \mathrm{O}=16\right]$

What mass of oxygen is there in $174 \mathrm{g}$ of manganese oxide?

$110 \mathrm{g}$ of manganese was extracted from $174 \mathrm{g}$ of manganese oxide. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Mn}=55, \mathrm{O}=16\right]$

How many moles of oxygen atoms are there in $174 \mathrm{g}$ of manganese oxide?

$110 \mathrm{g}$ of manganese was extracted from $174 \mathrm{g}$ of manganese oxide. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Mn}=55, \mathrm{O}=16\right]$

$110 \mathrm{g}$ of manganese was extracted from $174 \mathrm{g}$ of manganese oxide. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Mn}=55, \mathrm{O}=16\right]$

$110 \mathrm{g}$ of manganese was extracted from $174 \mathrm{g}$ of manganese oxide. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{Mn}=55, \mathrm{O}=16\right]$

Find the molecular formulae for the compound given below. $\left[{\mathrm{A}}_{\mathrm{r}}: \mathrm{H}= 1, \mathrm{C}=12, \mathrm{N}=14, \mathrm{O}=16\right]$