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(A) The chemical equation for alcoholic fermentation is: $C_6H_{12}O_6 \rightarrow 2C_2H_5OH + 2CO_2$.According to the stoichiometry of the reaction,

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$0.3$

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(A) The chemical equation for alcoholic fermentation is: $C_6H_{12}O_6 \rightarrow 2C_2H_5OH + 2CO_2$.According to the stoichiometry of the reaction, $1$ mole of glucose produces $2$ moles of ethanol $(C_2H_5OH)$ and $2$ moles of carbon dioxide $(CO_2)$.The molar mass of ethanol is approximately $46 \, g/mol$, and the molar mass of $CO_2$ is approximately $44 \, g/mol$.Since the molar masses are very similar, in terms of mass, the production of ethanol and $CO_2$ occurs in a nearly $1:1$ ratio during fermentation.Therefore, if $0.3$ tonne of alcohol is produced, approximately $0.3$ tonne of $CO_2$ is released into the atmosphere.

$A$ brewery subjects about $1$ tonne of purified jaggery to fermentation under ideal conditions. If it has produced $0.3$ tonne of alcohol, what quantity of $CO_2$ has it expelled into the atmosphere (in $tonne$)?

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