Ramendra C Mukerjee Solutions for Chapter: Problems Based on Equations: Stoichiometry, Exercise 1: PROBLEMS

Equal weights of mercury and iodine are allowed to react completely to form a mixture of mercurous and mercuric iodide leaving none of the reactants. Calculate the ratio by weight of undefined and undefined formed.

$3.90 \mathrm{g}$ of a mixture of $\mathrm{Al}$ and ${\mathrm{Al}}_2{\mathrm{O}}_3$ when reacted with a solution of sodium hydroxide produced $840 \mathrm{mL}$ of a gas at $\mathrm{NTP}$. Find the composition of the mixture.

[Hint: Only $\mathrm{Al}$ produces ${\mathrm{H}}_2$]

One litre of an acidified solution of ${\mathrm{KMnO}}_4$ containing $15.8 \mathrm{g}$ of ${\mathrm{KMnO}}_4$ is decolourised by passing a sufficient amount of ${\mathrm{SO}}_2$. If ${\mathrm{SO}}_2$ is produced by roasting of iron pyrites $\left({\mathrm{FeS}}_2\right)$, what will be the amount of pyrites (in grams) required to produce the necessary amount of ${\mathrm{SO}}_2$?

(Atomic mass of $\mathrm{K}=39, \mathrm{Mn}=55, \mathrm{S}=32, \mathrm{O}=16, \mathrm{Fe}=56, \mathrm{H}=1$)

Round off your answer to the nearest integer.

When a mixture of $\mathrm{NaBr}$ and $\mathrm{NaCl}$ is repeatedly digested with sulphuric acid, all the halogens are expelled and ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is formed quantitatively. With a particular mixture, it was found that the weight of ${\mathrm{Na}}_2{\mathrm{SO}}_4$ obtained was precisely the same as the weight of $\mathrm{NaBr}-\mathrm{NaCl}$ mixture taken. Calculate the ratio of the weights of $\mathrm{NaCl}$ and $\mathrm{NaBr}$ in the mixture.

Give the final answer up to two places of decimal.

$25.4 \mathrm{g}$ of iodine and $14.2 \mathrm{g}$ of chlorine are made to react completely to yield a mixture of $\mathrm{ICl}$ and ${\mathrm{ICl}}_3$. Calculate the number of moles of $\mathrm{ICl}$ and ${\mathrm{ICl}}_3$ formed.

An alloy of aluminium and copper was treated with aqueous $\mathrm{HCl}$. The aluminium dissolved according to the reaction $\mathrm{Al}+3{\mathrm{H}}^{+}\to {\mathrm{Al}}^{3+}+\frac{3}{2}{\mathrm{H}}_2$, but the copper remained as a pure metal. A $0.350 \mathrm{g}$ sample of the alloy gave $415 \mathrm{cc}$ of ${\mathrm{H}}_2$ measured at $273 \mathrm{K}$ and $1 \mathrm{atm}$ pressure. What is the weight percentage of $\mathrm{Al}$ in the alloy?

Give the final answer up to first place of decimal after rounding off.

What weights of ${\mathrm{P}}_4{\mathrm{O}}_6$ and ${\mathrm{P}}_4{\mathrm{O}}_{10}$ will be produced by the combustion of $2 \mathrm{g}$ of ${\mathrm{P}}_4$ in $2 \mathrm{g}$ of ${\mathrm{O}}_2$, leaving no ${\mathrm{P}}_4$ and ${\mathrm{O}}_2$?

A mixture containing ${\mathrm{KClO}}_3, {\mathrm{KHCO}}_3, {\mathrm{K}}_2{\mathrm{CO}}_3$ and $\mathrm{KCl}$ was heated, producing ${\mathrm{CO}}_2, {\mathrm{O}}_2$ and ${\mathrm{H}}_2\mathrm{O}$ gases according to the following equations:

$$\begin{gathered} 2{\mathrm{KClO}}_3 \left(\mathrm{s}\right)\to 2\mathrm{KCl} \left(\mathrm{s}\right)+3{\mathrm{O}}_2 \\ 2{\mathrm{KHCO}}_3 \left(\mathrm{s}\right)\to {\mathrm{K}}_2\mathrm{O} \left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{O} \left(\mathrm{g}\right)+2{\mathrm{CO}}_2 \left(\mathrm{g}\right) \\ {\mathrm{K}}_2{\mathrm{CO}}_3 \left(\mathrm{s}\right)\to {\mathrm{K}}_2\mathrm{O} \left(\mathrm{s}\right)+{\mathrm{CO}}_2 \left(\mathrm{g}\right) \end{gathered}$$