NCERT Solutions for Chapter: Some Basic Concepts of Chemistry, Exercise 1: Short Answer Type

$45.4 \mathrm{L}$ of dinitrogen reacted with $22.7 \mathrm{L}$of dioxygen and $45.4 \mathrm{L}$ of nitrous oxide was formed. The reaction is given below:
$2{\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \to 2{\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)$
Which law is being obeyed in this experiment? Write the statement of the law?

If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element, are in whole number ratio.

(a) Is this statement true?

(b) If yes, according to which law?

(c) Give one example related to this law.

Calculate the average atomic mass of hydrogen using the following data:

Hydrogen gas is prepared In the laboratory by reacting dilute $\mathrm{HCl}$ with granulated zinc. Following reaction takes place.

$\mathrm{Zn}+2\mathrm{HCl}\to {\mathrm{ZnCl}}_2+{\mathrm{H}}_2$

Calculate the volume of hydrogen gas liberated at STP when $32.65 \mathrm{g}$ of zinc reacts with $\mathrm{HCl}$. $1 \mathrm{mol}$ of a gas occupies $22.7 \mathrm{L}$volume at STP; atomic mass of $\mathrm{Zn} = 65.3 \mathrm{u}.$

The density of 3 molal solution of $\mathrm{NaOH}$is $1.110 \mathrm{g} {\mathrm{mL}}^{-1}$. Calculate the molarity of the solution.

Volume of a solution changes with change in temperature, then, will the molality of the solution, be affected by temperature? Give reason for your answer.

If $4 \mathrm{g}$of $\mathrm{NaOH}$dissolves in $36 \mathrm{g}$of ${\mathrm{H}}_2\mathrm{O}$, calculate the mole fraction of each component in the solution. Also, determine the molarity of solution (specific gravity of solution is $1\mathrm{g} {\mathrm{mL}}^{-1}$).

The reactant which is entirely consumed in reaction is known as limiting reagent. In the reaction$2\mathrm{A}+4\mathrm{B}\to 3\mathrm{C}+4\mathrm{D}$. when $5$ moles of A react with $6$ moles of B, then

(i) which is the limiting reagent?

(ii) calculate the amount of C formed.