What is the mass of one mole of water ($H_2O$)? (Atomic masses: H = 1u, O = 16u)

A 1.00 g sample containing $BaCl_2\cdot2H_2O$ is heated to a constant mass of 0.835 g. What was the mass percent of barium in the original sample?

How many milligram of iron (${\rm{(F}}{{\rm{e}}^{2 + }})$ are equal to 1 mL of 0.1055 $N{{\rm{K}}_2}{\rm{C}}{{\rm{r}}_2}{{\rm{O}}_7}$equivalent?

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?

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 limiting reagent when 2 moles of $H_2$ react with 1 mole of $O_2$ to form water?

In an experiment during the analysis of a carbon compound, $145\,\,{\rm{mL of}}\,\,{{\rm{H}}_2}$ was collected at $760\,\,{\rm{mm Hg}}$ pressure and ${27^0}C$. The weight of ${H_2}$ is nearly :

20g of hydrogen gas reacts with 40g of oxygen to produce water. Which is the limiting reagent and how much water is formed(in grams)?

How many milligram of iron (${\rm{(F}}{{\rm{e}}^{2 + }})$ are equal to 1 mL of 0.1055 $N{{\rm{K}}_2}{\rm{C}}{{\rm{r}}_2}{{\rm{O}}_7}$equivalent?

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 $\mathrm{Ca} = 40$)

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