Calculate the number of atoms in 0.5 moles of sulfur (S). (Avogadro's Number = $6.022 imes 10^{23}$)

Calculate the number of moles of $\mathrm{CO_2}$ produced when 50 g of calcium carbonate containing 60% impurity is completely decomposed upon heating. (Atomic mass of $\mathrm{Ca} = 40$)

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

A chemical balance used normally for weighing in laboratory can weigh upto a least count of :

10 g of calcium carbonate ($CaCO_3$) on heating produces how many grams of calcium oxide ($CaO$)? (Atomic masses: Ca = 40, C = 12, O = 16)

How many moles of $CO_2$ are produced when 2 moles of propane ($C_3H_8$) are completely combusted in excess oxygen?

What weight of ${\rm{FeS}}{{\rm{O}}_4}$ (mol. wt. =152) will be oxidised by 200 mL of normal ${\rm{KMn}}{{\rm{O}}_4}$ solution in acidic solution?

What volume of 2$N$ ${{\rm{K}}_2}{\rm{C}}{{\rm{r}}_2}{{\rm{O}}_7}$ solution is required to oxidise 0.81 g of ${{\rm{H}}_2}{\rm{S}}$ in acidic medium?

2 mole of ${\rm{FeS}}{{\rm{O}}_4}$ are oxidized by 'X' mole of ${\rm{KMn}}{{\rm{O}}_4}$ whereas 2 mole of ${\rm{Fe}}{{\rm{C}}_2}{{\rm{O}}_4}$ are oxidized by 'Y' mole of ${\rm{KMn}}{{\rm{O}}_4}$. The ration f 'X' and 'Y' is :

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

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 :

Volume of $C{O_2}$ produced on heating 10 g of limestone at S.T.P