A mixture of $KClO_3$ and $KCl$ weighing 4.96 g was heated to produce $O_2$. The evolved oxygen occupied 448 mL at STP. What percent of the original mixture was $KClO_3$?

A 10g sample of $CaC{O_3}$ with 80% purity was heated to a constant weight volume of $C{O_2}$ gas liberated under STP conditions is approximately

How many milliliter of 0.5 $N$ ${\rm{SnC}}{{\rm{l}}_2}$ solution will reduce 600 mL of 0.1 $N$ ${\rm{HgC}}{{\rm{l}}_2}$ to ${\rm{H}}{{\rm{g}}_2}{\rm{C}}{{\rm{l}}_2}$?

A 0.518 g sample of lime stone is dissolved in $HCl$ and then the calcium is precipitated as ${\rm{Ca}}{{\rm{C}}_2}{{\rm{O}}_4}$. After filtering and washing the precipitate, it requires 40.0 mL of $0.250N{\rm{KMn}}{{\rm{O}}_4},$, solution acidified with ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}$ to titrate is as, ${\rm{MnO}}_4^ - + {{\rm{H}}^ + } + {{\rm{C}}_2}{\rm{O}}_4^{2 - } o {\rm{M}}{{\rm{n}}^{2 + }} + {\rm{C}}{{\rm{O}}_2} + 2{{\rm{H}}_2}{\rm{O}}$. The percentage of ${\rm{CaO}}$ in the sample is :

0.9 g Al reacts with dil. $HCl$ to give ${H_2}$ . The volume of ${H_2}$ evolved at STP is

Upon heating 20 g of limestone with 20% purity, what mass of $\mathrm{CO_2}$ is produced? (Atomic mass of $\mathrm{Ca} = 40$)

$\left[\mathrm{CaCO_3} \stackrel{1200 \mathrm{K}}{\longrightarrow} \mathrm{CaO} + \mathrm{CO_2}\right]$

What is the Mass of one molecule of yellow Phosphorous (Atomic Mass = 30)

The equivalent weight of ${\rm{KMn}}{{\rm{O}}_4}$ (acidic medium) is (at. wt. of K = 39; $Mn$ = 55) :

30 g of impure marble chips containing 80% $\mathrm{CaCO_3}$ is heated strongly. Calculate the mass of $\mathrm{CaO}$ formed. (Atomic masses: $\mathrm{Ca} = 40$, $\mathrm{C} = 12$, $\mathrm{O} = 16$)

$\mathrm{CaCO_3} \rightarrow \mathrm{CaO} + \mathrm{CO_2}$

How many moles are present in 32g of oxygen gas ($O_2$)? (Atomic mass of O = 16u)

The equivalent weight of ${\rm{KMn}}{{\rm{O}}_4}$ (acidic medium) is (at. wt. of K = 39; $Mn$ = 55) :