Mole Concept

To a $25 \mathrm{ml} {\mathrm{H}}_2{\mathrm{O}}_2$ solution excess acidified solution of $\mathrm{Kl}$ was added. The iodine liberated $20 \mathrm{ml}$ of $0.3 \mathrm{N}$ sodium this sulphate solution. Use these data to choose the correct statements from the following :

How many millilitres of $0.1 \mathrm{N} {\mathrm{H}}_2{\mathrm{SO}}_4$ solution will be required for complete reaction with a solution containing $0.125 \mathrm{g}$ of pure ${\mathrm{Na}}_2{\mathrm{CO}}_3$ :

When $1 \mathrm{mole}$ of A reacts with $\frac{1}{2}\mathrm{mole}$ of B_{2$\left(\mathrm{A}+\frac{1}{2}{\mathrm{B}}_2\to \mathrm{AB}\right)$}, $100 \mathrm{kcal}$ heat is liberated and when $1 \mathrm{mole}$ of A reacted with $2 \mathrm{mole}$ of B₂ $\left(\mathrm{A}+2{\mathrm{B}}_2\to {\mathrm{AB}}_4\right)$, $200 \mathrm{kcal}$ heat is liberated. When of A is completely reacted with excess of B₂ to form AB as well as AB₄, $140 \mathrm{kcal}$ heat is liberated. Calculate the mole of B₂ used. [Write your answer as number of mole of B₂ used $\times 10$].

How many moles of magnesium phosphate, $\mathrm{Mg}{\left({\mathrm{PO}}_4\right)}_2$ will contain $0.25$mole of oxygen atoms? 

$21.2 \mathrm{g}$ sample of impure ${\mathrm{Na}}_2{\mathrm{CO}}_3$ is dissolved and reacted with a solution of ${\mathrm{CaCl}}_2,$ the weight of precipitate of ${\mathrm{CaCO}}_3$ is $10.0 \mathrm{g}$. Which of the following statements is/are correct? 

$100 \mathrm{g}$ sample of clay (containing $19\% {\mathrm{H}}_2\mathrm{O}, 40\%$ silica, and inert impurities as rest) is partially dried to contain $10\% {\mathrm{H}}_2\mathrm{O}$.
Which of the following is/are correct statements (s)?

For the following reaction:

${\mathrm{Na}}_2{\mathrm{CO}}_3+2\mathrm{HCl}⟶2\mathrm{NaCl}+{\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}$
$106.0\mathrm{g}$ of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ reacts with$109.5\mathrm{g}$ of $\mathrm{HCl}$
Which of the following is/are correct.

A sample of a mixture of ${\mathrm{CaCl}}_2$ and $\mathrm{NaCl}$ weighing $4.44 \mathrm{g}$ was treated to precipitate all the $\mathrm{Ca}$ as ${\mathrm{CaCO}}_3,$ which was then heated and quantitatively converted to $1.12 \mathrm{g}$ of $\mathrm{CaO}$.

(At.wt: $\mathrm{Ca}=40,\mathrm{Na}=23,\mathrm{Cl}=35.5$)

(i) ${\mathrm{K}}_4\mathrm{Fe}(\mathrm{CN}{)}_6+3{\mathrm{H}}_2{\mathrm{SO}}_4⟶2{\mathrm{K}}_2{\mathrm{SO}}_4+{\mathrm{FeSO}}_4+6\mathrm{HCN}$

(ii) $6\mathrm{HCN}+12{\mathrm{H}}_2\mathrm{O}⟶6\mathrm{HCOOH}+6{\mathrm{NH}}_3$

(iii) (a) $6{\mathrm{NH}}_3+3{\mathrm{H}}_2{\mathrm{SO}}_4⟶3{\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4$
(b) $6\mathrm{HCOOH}\stackrel{{\mathrm{H}}_2{\mathrm{SO}}_4}{\to }6\mathrm{CO}+6{\mathrm{H}}_2\mathrm{O}$

Above steps of reactions occur in a container starting with one ${\mathrm{K}}_4\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right],5$ mole of ${\mathrm{H}}_2{\mathrm{SO}}_4$ and enough water. Find out the limiting reagent in step (i) and calculate maximum moles of $\mathrm{CO}$ gas and ${\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4$ that can be produced.

Which is/are correct statements about $1.7\mathrm{g}$ of ${\mathrm{NH}}_3:$

$92 \mathrm{g}$ mixture of ${\mathrm{CaCO}}_3$, and ${\mathrm{MgCO}}_3$ heated strongly in an open vessel. After complete decomposition of the carbonates it was found that the weight of residue left behind is $48 \mathrm{g}$. Find the mass of ${\mathrm{MgCO}}_3$ in grams in the mixture.

If $240 \mathrm{g}$ of carbon is taken in a container to convert it completely to ${\mathrm{CO}}_2$ but in industry it has been found that $280 \mathrm{g}$ of $\mathrm{CO}$ was also formed along with ${\mathrm{CO}}_2$. Find the mole percentage yield of ${\mathrm{CO}}_2$. The reactions occurring are:

$\mathrm{C}+{\mathrm{O}}_2⟶{\mathrm{CO}}_2;\mathrm{C}+\frac{1}{2}{\mathrm{O}}_2⟶\mathrm{CO}$

A sample of Calcium phosphate ${\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2$ contains $8 \mathrm{mole}$ of $\mathrm{O}$ atoms. The number of $\mathrm{mol}$ of $\mathrm{Ca}$ atoms in the sample is:

How many moles of potassium chlorate need to be heated to produce $11.2$litre oxygen at $\mathrm{N}.\mathrm{T}.\mathrm{P}.$

How many liters of ${\mathrm{CO}}_2$ at $\mathrm{STP }$will be formed when $0.01\mathrm{mol}$  of  ${\mathrm{H}}_2{\mathrm{SO}}_4$reacts with excess of ${\mathrm{Na}}_2{\mathrm{CO}}_3$?

${\mathrm{Na}}_2{\mathrm{CO}}_3+{\mathrm{H}}_2{\mathrm{SO}}_4⟶{\mathrm{Na}}_2{\mathrm{SO}}_4+{\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}$

A sample of chalk contains clay as an impurity. The clay impurity loses $11\%$ of its weight as moisture on prolong heating. $5$ gram sample of chalk on heating shows a loss in weight (due to the evolution of ${\mathrm{CO}}_2$ and water) by $1.1\mathrm{g}.$ Calculate the $\%$ of chalk $\left({\mathrm{CaCO}}_3\right)$ in the sample. [Hint : Chalk $\left({\mathrm{CaCO}}_3\right)$ release ${\mathrm{CO}}_2$ on heating]

A $2\mathrm{g}$ sample containing ${\mathrm{Na}}_2{\mathrm{CO}}_3$ and ${\mathrm{NaHCO}}_3$looses $0.248\mathrm{g}$ when heated to $300°\mathrm{C}$ , the temperature at which ${\mathrm{NaHCO}}_3$ decomposes to ${\mathrm{Na}}_2{\mathrm{CO}}_3, {\mathrm{CO}}_2$ and ${\mathrm{H}}_2\mathrm{O}$. What is the percentage of ${\mathrm{Na}}_2{\mathrm{CO}}_3$ in the given mixture?

${\mathrm{KCIO}}_3$ decomposes by two parallel reactions,

($i$) $2{\mathrm{KClO}}_3\stackrel{\Delta }{⟶}2\mathrm{KCl}+3{\mathrm{O}}_2$  ($ii$) $4{\mathrm{KClO}}_3\stackrel{\Delta }{⟶}3{\mathrm{KClO}}_4+\mathrm{KCl}$

If $3$ moles of ${\mathrm{O}}_2$ and$1\mathrm{mol}$ of ${\mathrm{KClO}}_4$ is produced along with other products, then determine the initial moles of ${\mathrm{KClO}}_3$.

The percent yield for the following reaction carried out in carbon tetrachloride $\left({\mathrm{CCl}}_4\right)$ solution is $80\%$.

${\mathrm{Br}}_2+{\mathrm{Cl}}_2⟶2\mathrm{BrCl}$

(a) What amount of $\mathrm{BrCl}$ would be formed from the reaction of $0.025 \mathrm{mol} {\mathrm{Br}}_2$ and $0.025 \mathrm{mol} {\mathrm{Cl}}_2$?
(b) What amount of ${\mathrm{Br}}_2$ is left unchanged?

$50 \mathrm{g}$ of ${\mathrm{CaCO}}_3$ is allowed to react with $73.5 \mathrm{g}$ of ${\mathrm{H}}_3{\mathrm{PO}}_4$. Calculate the following in moles:
($\mathrm{i}$) Amount of ${\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2$ formed
($\mathrm{ii}$) Amount of unreacted reagent