Define the Law of Conservation of Mass.
(N/A) The Law of Conservation of Mass states that matter can neither be created nor destroyed in a chemical reaction.
This law was put forth by Antoine Lavoisier in $1789$.
He performed careful experimental studies for combustion reactions to reach this conclusion.
This law formed the basis for several later developments in chemistry.
It is the result of exact measurements of the masses of reactants and products in carefully planned experiments.
This law was put forth by Antoine Lavoisier in $1789$.
He performed careful experimental studies for combustion reactions to reach this conclusion.
This law formed the basis for several later developments in chemistry.
It is the result of exact measurements of the masses of reactants and products in carefully planned experiments.
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Similar Questions
Gay-Lussac's law of gaseous volumes is derived from $.......$.
Easy
View SolutionThe following data are obtained when dinitrogen and dioxygen react together to form different compounds:
Mass of dinitrogen Mass of dioxygen $(i) \ 14 \ g$ $16 \ g$ $(ii) \ 14 \ g$ $32 \ g$ $(iii) \ 28 \ g$ $32 \ g$ $(iv) \ 28 \ g$ $80 \ g$
$(a)$ Which law of chemical combination is obeyed by the above experimental data? Give its statement.
$(b)$ Fill in the blanks in the following conversions:
$(i) \ 1 \ km = \dots \ mm = \dots \ pm$
$(ii) \ 1 \ mg = \dots \ kg = \dots \ ng$
$(iii) \ 1 \ mL = \dots \ L = \dots \ dm^{3}$
| Mass of dinitrogen | Mass of dioxygen |
|---|---|
| $(i) \ 14 \ g$ | $16 \ g$ |
| $(ii) \ 14 \ g$ | $32 \ g$ |
| $(iii) \ 28 \ g$ | $32 \ g$ |
| $(iv) \ 28 \ g$ | $80 \ g$ |
$(a)$ Which law of chemical combination is obeyed by the above experimental data? Give its statement.
$(b)$ Fill in the blanks in the following conversions:
$(i) \ 1 \ km = \dots \ mm = \dots \ pm$
$(ii) \ 1 \ mg = \dots \ kg = \dots \ ng$
$(iii) \ 1 \ mL = \dots \ L = \dots \ dm^{3}$
Difficult
View SolutionIn compound $A$,$1.00 \, g$ nitrogen unites with $0.57 \, g$ oxygen. In compound $B$,$2.00 \, g$ nitrogen combines with $2.24 \, g$ oxygen. In compound $C$,$3.00 \, g$ nitrogen combines with $5.11 \, g$ oxygen. These results obey the following law:
Medium
View SolutionThe statement related to the law of definite proportions is:
$1 \, L$ of $N_2$ combines with $3 \, L$ of $H_2$ to form $2 \, L$ of $NH_3$ under the same conditions. This illustrates the:
Difficult
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