(B) The combustion reaction is: $2H_2(g) + O_2(g) \rightarrow 2H_2O(l)$.Given $4 \ g$ of $H_2$ $(n = 4/2 = 2 \ mol)$, it produces $2 \ mol$ of $H_2O$.

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(B) The combustion reaction is: $2H_2(g) + O_2(g) \rightarrow 2H_2O(l)$.Given $4 \ g$ of $H_2$ $(n = 4/2 = 2 \ mol)$, it produces $2 \ mol$ of $H_2O$.The density of water is $1 \ g/mL$, so the volume of $2 \ mol$ of $H_2O$ $(36 \ g)$ is $36 \ mL = 36 \times 10^{-3} \ L$.The amount of $CO_2$ is $36 \ \mu mol = 36 \times 10^{-6} \ mol$.Concentration of $CO_2 = \frac{n}{V} = \frac{36 \times 10^{-6} \ mol}{36 \times 10^{-3} \ L} = 10^{-3} \ M = 1 \ mM$.

Class 11 Chemistry Some Basic Concepts of Chemistry Chemical stoichiometry

Medium

While combusting in air, $4 \ g$ of $H_2$ gas was completely converted into water. If $36 \ \mu mole$ of $CO_2$ from air is dissolved into that water, what is the concentration of $CO_2$?

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A
$1 \ \mu M$
B
$1 \ mM$
C
$1 \ nM$
D
$1000 \ mM$

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Class 11

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Some Basic Concepts of Chemistry

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Chemical stoichiometry

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While combusting in air, $4 \ g$ of $H_2$ gas was completely converted into water. If $36 \ \mu mole$ of $CO_2$ from air is dissolved into that water, what is the concentration of $CO_2$?

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