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(D) The balanced chemical equation is: $CS_2 + 3O_2 	o 2SO_2 + CO_2$.Analysis of options:$(A)$ From the stoichiometry,$1 \ mole$ of $CS_2$ produces $

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Six molecules of oxygen requires three molecules of $CS_2$

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(D) The balanced chemical equation is: $CS_2 + 3O_2 	o 2SO_2 + CO_2$.Analysis of options:$(A)$ From the stoichiometry,$1 \ mole$ of $CS_2$ produces $1 \ mole$ of $CO_2$. This is true.$(B)$ Molar mass of $O_2 = 32 \ g/mol$. $16 \ g$ of $O_2 = 0.5 \ mol$. From the equation,$3 \ mol$ of $O_2$ produces $1 \ mol$ of $CO_2$ $(44 \ g)$. So,$0.5 \ mol$ of $O_2$ produces $(1/3) 	imes 0.5 	imes 44 \approx 7.33 \ g$ of $CO_2$. This is true.$(C)$ From the equation,$3 \ mol$ of $O_2$ produces $2 \ mol$ of $SO_2$. Therefore,$1 \ mol$ of $O_2$ produces $2/3 \ mol$ of $SO_2$. This is true.$(D)$ From the equation,$3 \ molecules$ of $O_2$ react with $1 \ molecule$ of $CS_2$. Thus,$6 \ molecules$ of $O_2$ require $2 \ molecules$ of $CS_2$,not $3$. This statement is false.

Which statement is false for the balanced equation given below?
$CS_2 + 3O_2 \to 2SO_2 + CO_2$

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Which statement is false for the balanced equation given below?$CS_2 + 3O_2 \to 2SO_2 + CO_2$