State and explain Gay-Lussac's Law of Gaseous Volumes.
This law was proposed by Gay-Lussac in $1808$.
He observed that when gases combine or are produced in a chemical reaction,they do so in a simple ratio by volume,provided all gases are at the same temperature and pressure.
For example,$100 \ mL$ of hydrogen combines with $50 \ mL$ of oxygen to give $100 \ mL$ of water vapour.
$\text{Hydrogen} + \text{Oxygen} \rightarrow \text{Water vapour}$
$100 \ mL$ $50 \ mL$ $100 \ mL$
Thus,the volumes of hydrogen and oxygen which combine together (i.e.,$100 \ mL$ and $50 \ mL$) bear a simple ratio of $2:1$.
Gay-Lussac's discovery of an integer ratio in volume relationships is essentially the law of definite proportions by volume,whereas the earlier law was with respect to mass.
He observed that when gases combine or are produced in a chemical reaction,they do so in a simple ratio by volume,provided all gases are at the same temperature and pressure.
For example,$100 \ mL$ of hydrogen combines with $50 \ mL$ of oxygen to give $100 \ mL$ of water vapour.
$\text{Hydrogen} + \text{Oxygen} \rightarrow \text{Water vapour}$
$100 \ mL$ $50 \ mL$ $100 \ mL$
Thus,the volumes of hydrogen and oxygen which combine together (i.e.,$100 \ mL$ and $50 \ mL$) bear a simple ratio of $2:1$.
Gay-Lussac's discovery of an integer ratio in volume relationships is essentially the law of definite proportions by volume,whereas the earlier law was with respect to mass.
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Similar Questions
To check the principle of multiple proportions,a series of pure binary compounds $(P_m Q_n)$ were analyzed and their composition is tabulated below. The correct option$(s)$ is(are)
Compound Weight $\%$ of $P$ Weight $\%$ of $Q$ $1$ $50$ $50$ $2$ $44.4$ $55.6$ $3$ $40$ $60$
$(A)$ If empirical formula of compound $3$ is $P_3 Q_4$,then the empirical formula of compound $2$ is $P_3 Q_5$.
$(B)$ If empirical formula of compound $3$ is $P_3 Q_2$ and atomic weight of element $P$ is $20$,then the atomic weight of $Q$ is $45$.
$(C)$ If empirical formula of compound $2$ is $PQ$,then the empirical formula of the compound $1$ is $P_5 Q_4$.
$(D)$ If atomic weight of $P$ and $Q$ are $70$ and $35$,respectively,then the empirical formula of compound $1$ is $P_2 Q$.
| Compound | Weight $\%$ of $P$ | Weight $\%$ of $Q$ |
| $1$ | $50$ | $50$ |
| $2$ | $44.4$ | $55.6$ |
| $3$ | $40$ | $60$ |
$(A)$ If empirical formula of compound $3$ is $P_3 Q_4$,then the empirical formula of compound $2$ is $P_3 Q_5$.
$(B)$ If empirical formula of compound $3$ is $P_3 Q_2$ and atomic weight of element $P$ is $20$,then the atomic weight of $Q$ is $45$.
$(C)$ If empirical formula of compound $2$ is $PQ$,then the empirical formula of the compound $1$ is $P_5 Q_4$.
$(D)$ If atomic weight of $P$ and $Q$ are $70$ and $35$,respectively,then the empirical formula of compound $1$ is $P_2 Q$.
If element $A$ combines with element $B$ in a ratio of $1:2$ by mass,and element $A$ combines with element $C$ in a ratio of $6:4$ by mass,then by which law do elements $B$ and $C$ combine with each other?
Medium
View SolutionWhich of the following examples illustrates the Law of Multiple Proportions?
Easy
View SolutionWhich law is followed by the different proportions of oxygen in various oxides of nitrogen?
Easy
View SolutionWho proposed the Law of Multiple Proportions?
Easy
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