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How does the reaction of Sodium hydrogen carbonate and hydrochloric acid support the theory of conservation of mass?

Last updated date: 20th Jun 2024
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Hint: The Law of Conservation of Mass is defined and explained using examples of reacting mass calculations using the law are fully explained with worked out examples using the balanced symbol equation. The process involves reacting masses deduced from the balanced symbol equation.

Complete step by step answer:
In a word, the mass of the entirety of the gases evolved and the mass of the aqueous remains- combined- shall be equivalent to the amount of the mass of the two reactants.
Sodium bicarbonate \[NaHC{O_3}\] and hydrochloric acid \[HCl\] react to form sodium chloride, water, and carbon dioxide-an unscented gas-by the condition
\[NaHC{O_3}\] \[\left( {aq} \right)\] \[ + \] \[HCl\] \[\left( {aq} \right)\] -----> \[Nacl\] \[ + \] \[{H_2}O\] \[\left( l \right)\]\[\; + \] \[C{O_2}\left( g \right)\]
The mass of the system won't ration if the response happens in an open container: carbon dioxide escapes quickly as the response continues, with the end goal that the mass of the products would be more modest than that of the reactants:
\[m{\text{ }}\left( {{\text{ }}reactants{\text{ }}} \right)\] =\[m\left( {products} \right)\]
=\[m\left( {Aqueous{\text{ }}left - over} \right)\] + \[m\left( {C{O_2}} \right)\]
\[m{\text{ }}\left( {{\text{ }}reactants{\text{ }}} \right)\] \[m{\text{ }}\left( {Aqueous{\text{ }}left - over{\text{ }}} \right)\]
Checking the preservation of mass for this reaction would, hence, require trapping all gases delivered inside the system. A conical flask with an air-tight stopper is likely going to fill the need.

Given the way that most electronic adjusts found in science labs are aligned at room temperature and the exothermic nature of the reaction, it very well may be important to cool the system down to its initial temperature prior to taking any further estimations.