Question

Avogadro’s law shows the relationship between which two variables?
(A) Volume and number of moles
(B) Pressure and number of moles
(C) Volume and pressure
(D) Temperature and Pressure
(E) Temperature and number of moles

Answer 1

Avogadro’s Law states that at constant temperature and pressure, equal volume of all gases contain equal numbers of atoms. Thus, it is evident that Avogadro’s law shows the relationship between these two variables.

Complete step by step answer:
First of all let us understand about autogiro law. This law was proposed by Swedish chemist Berzelius. This law starter that equal volumes of all gases under pressure contain equal number of atom/molecule are mole,
For example consider a reaction
${H_2} + C{l_2} \to 2HCl$
From this equation we got to know that volume of reacts with volume of to give 2 volumes of $HCl$ or 1male of H reacts with 1mole of cl to give moles of $HCl$ this observation is accreting to avogadro law
A Avogadro law also states that gases at constant pressure and constant temperature volume are directly proportional to the no of moles of gas present in the vessel.
$i.e$ $v\alpha n$ [n=no of molar of gores]
At and one atmospheres pressure the one male of all gases occupy 22.4l of volume. Moreover from Avogadro law we can serve the relation between molar mass and density of gore.
According to Avogadro law $v\alpha n$ or $v = kn$ here k is a content of proportionally.
We also know that no of molars = $n\dfrac{m}{M}$ Where m is the given mass and m is the molar mass of the gas.
We know that density = $d = \dfrac{m}{v},$so the
Above equation we become
$M = Kd$ or $M\alpha d$
Hence we conclude that density of a gas is directly proportional to its molar mass.

Hence option (A) is the correct answer .

Note:
The avogadro law is also the basis of the mole concept as it explains the relation between the number of gas molecules and the volume , temperature and pressure corresponding to it.