Stoichiometry Questions

Among the following, choose the ones with equal number of atoms:A. $212\text{g}$ of ${\text{Na}}_2{\text{CO}}_3$ ($\text{s}$) [molar mass = $106\text{g}$ ]B. $248\text{g}$ of ${\text{Na}}_2\text{O}$ ($\text{s}$) [molar mass = $62\text{g}$ ]C. $240\text{g}$ of $\text{NaOH}$ ($\text{s}$) [molar mass = $40\text{g}$ ]D. $12\text{g}$ of ${\text{H}}_2$ ($\text{g}$) [molar mass = $2\text{g}$ ]E. $220\text{g}$ of ${\text{CO}}_2$ ($\text{g}$) [molar mass = $44\text{g}$ ]Choose the correct answer from the options given below:

In the balanced chemical reaction${\text{IO}}_3^{-}+a{\text{I}}^{-}+b{\text{H}}^{+}\to c{\text{H}}_2\text{O}+d{\text{I}}_2$$a,b,c$ and $d$ respectively corresponds to:

The number of moles of ${\text{KMnO}}_4$ that will be needed to react with one mole of sulphite ion in acidic solution is:

What volume of oxygen gas (${\text{O}}_2$) measured at $0^{\circ }\text{C}$ and $1\text{atm}$, is needed to burn completely $1\text{L}$ of propane gas (${\text{C}}_3{\text{H}}_8$) measured under the same conditions?

How many moles of lead (II) chloride will be formed from a reaction between $6.5\text{g}$ of $\text{PbO}$ and $3.2\text{g}$ of $\text{HCl}$?

Number of moles of ${\text{MnO}}_4^{-}$ required to oxidize one mole of ferrous oxalate completely in acidic medium will be:

$10\text{g}$ of hydrogen and $64\text{g}$ of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:

What is the $[{\text{OH}}^{-}]$ in the final solution prepared by mixing $20.0\text{mL}$ of $0.050\text{M HCl}$ with $30.0\text{mL}$ of $0.10{\text{M Ba(OH)}}_2$?

$25.3\text{g}$ of sodium carbonate, ${\text{Na}}_2{\text{CO}}_3$ is dissolved in enough water to make $250\text{mL}$ of solution. If sodium carbonate dissociates completely, molar concentration of sodium ion, ${\text{Na}}^{+}$ and carbonate ions, ${\text{CO}}_3^{2-}$ are respectively: (Molar mass of ${\text{Na}}_2{\text{CO}}_3=106{\text{g mol}}^{-1}$)

The number of atoms in $0.1\text{mol}$ of a triatomic gas is ($N_A=6.02\times 10^{23}{\text{mol}}^{-1}$):

How many grams of concentrated nitric acid solution (70% ${\text{HNO}}_3$ by mass) should be used to prepare $250\text{mL}$ of $2.0\text{M}$ ${\text{HNO}}_3$?

When $22.4\text{litres}$ of ${\text{H}}_2(g)$ is mixed with $11.2\text{litres}$ of ${\text{Cl}}_2(g)$, each at S.T.P., the moles of $\text{HCl}(g)$ formed is equal to:

$20.0\text{g}$ of a magnesium carbonate sample decomposes on heating to give carbon dioxide and $8.0\text{g}$ magnesium oxide. What will be the percentage purity of magnesium carbonate in the sample? (Atomic weight: $\text{Mg}=24$, $\text{C}=12$, $\text{O}=16$)

What is the mass of the precipitate formed when $50\text{mL}$ of $16.9\%$ solution of ${\text{AgNO}}_3$ is mixed with $50\text{mL}$ of $5.8\%$ $\text{NaCl}$ solution?

Suppose the elements $\text{X}$ and $\text{Y}$ combine to form two compounds ${\text{XY}}_2$ and ${\text{X}}_3{\text{Y}}_2$. When $0.1\text{mole}$ of ${\text{XY}}_2$ weighs $10\text{g}$ and $0.05\text{mole}$ of ${\text{X}}_3{\text{Y}}_2$ weighs $9\text{g}$, the atomic weights of $\text{X}$ and $\text{Y}$ are: