Stoichiometry and Stoichiometric Calculations

Calcium carbonate reacts with aqueous $\mathrm{HCl}$ to give ${\mathrm{CaCl}}_2$ and ${\mathrm{CO}}_2$ according to the reaction,
${\mathrm{CaCO}}_3\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)\to {\mathrm{CaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$.
What mass of ${\mathrm{CaCO}}_3$ is required to react completely with $25 \mathrm{mL}$ of $0.75 \mathrm{M} \mathrm{HCl}$?

In a reaction $\mathrm{A}+{\mathrm{B}}_2\to {\mathrm{AB}}_2$
Identify the limiting reagent, if any, in the following reaction mixture.
$2.5$ moles $\mathrm{A} + 5$ mole $\mathrm{B}$.

In a reaction $\mathrm{A}+{\mathrm{B}}_2\to {\mathrm{AB}}_2$
Identify the limiting reagent, if any, in the following reaction mixture.
$5$ mole $\mathrm{A}+2.5$ mole $\mathrm{B}$

In a reaction $\mathrm{A}+{\mathrm{B}}_2\to {\mathrm{AB}}_2$
Identify the limiting reagent, if any, in the following reaction mixture.
$100$ atoms of $\mathrm{A}+100$ molecules of $\mathrm{B}$

In a reaction $\mathrm{A}+{\mathrm{B}}_2\to {\mathrm{AB}}_2$
Identify the limiting reagent, if any, in the following reaction mixture.
$2$ moles of $\mathrm{A}+3$ moles of $\mathrm{B}$

In a reaction $\mathrm{A}+{\mathrm{B}}_2\to {\mathrm{AB}}_2$

Identify the limiting reagent, if any, in the following reaction mixture.
$300$ atoms of $\mathrm{A}+200$ molecules of $\mathrm{B}$

lf the density of methanol is $0.793 \mathrm{kg} {\mathrm{L}}^{-1}$, what is its volume needed for making $2.5 \mathrm{L}$ of its $0.25 \mathrm{M}$ solution?

(Provide correct answer upto two decimal places and no need to mention units).

In three moles of ethane $\left({\mathrm{C}}_2{\mathrm{H}}_6\right)$, calculate the following:

The number of molecules of ethane. 

In three moles of ethane $\left({\mathrm{C}}_2{\mathrm{H}}_6\right)$, calculate the following:

The number of moles of hydrogen atoms. 

In three moles of ethane $\left({\mathrm{C}}_2{\mathrm{H}}_6\right)$, calculate the following:

Number of moles of carbon atoms.
(Only mention the number, not the unit)

How much copper can be obtained (in 'g') from $100 \mathrm{g}$ of copper sulphate $\left({\mathrm{CuSO}}_4\right)$?
$\left[\mathrm{Atomic} \mathrm{weight} \mathrm{of} \mathrm{Cu}=63.5\right]$

$$\begin{gathered} \mathrm{A} : 36.8 \\ \mathrm{B} : 39.81 \\ \mathrm{C} : 49.81 \end{gathered}$$

Enter your correct answer as $\mathrm{A}, \mathrm{B} \mathrm{or} \mathrm{C}$.
 

Calculate and write the amount of carbon dioxide that could be produced (in $\mathrm{g}$) when $2$ moles of carbon is burnt in $16 \mathrm{g}$ of dioxygen. Choose the correct answer from the bracket: $\left(16\mathrm{g}, 22\mathrm{g}, 18\mathrm{g}\right)$

Calculate the amount of carbon dioxide that could be produced when,

$1$ mole of carbon is burnt in $16 \mathrm{g}$ of dioxygen.

$$\begin{gathered} \mathrm{A} : 0.01 \mathrm{moles} \\ \mathrm{B} : 0.5 \mathrm{moles} \\ \mathrm{C} : 0.1 \mathrm{moles} \end{gathered}$$

Enter your correct answer as $\mathrm{A}, \mathrm{B} \mathrm{or} \mathrm{C}$.

Calculate the amount of carbon dioxide (in moles) that could be produced when $1$ mole of carbon is burnt in air. 

Chlorine is prepared in the laboratory by treating manganese dioxide $\left({\mathrm{MnO}}_2\right)$ with aqueous hydrochloric acid according to the reaction

$4 \mathrm{HCl} \left(\mathrm{aq}\right) +{\mathrm{MnO}}_2 \left(\mathrm{s}\right) \to 2{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right) + {\mathrm{MnCl}}_2 \left(\mathrm{aq}\right) + {\mathrm{Cl}}_2\left(\mathrm{g}\right)$

How many grams of HCl react with $5.0 \mathrm{g}$ of manganese dioxide?

Calculate the number of atoms in each of the following (i) $52$ moles of $\mathrm{Ar}$ (ii) $52\mathrm{u}$ of $\mathrm{He}$ (iii) $52\mathrm{g}$ of $\mathrm{He}$.

Dinitrogen and dihydrogen react with each other to produce ammonia according to the following chemical reaction:
${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$
(i) Calculate the mass of ammonia produced if $2.00\times 10^3 \mathrm{g}$ dinitrogen reacts with $1.00\times 10^3 \mathrm{g}$ of dihydrogen.

(ii) Will any of the two reactants remain unreacted?

(iii) If yes, which one and what would be its mass?

Determine the empirical formula of an oxide of iron, which has $69.9\%$ iron and $30.1\%$ dioxygen by mass.