While combusting in air, 4 g of H 2 gas was completely converted into water. If 36 μ mole of CO 2 from air is dissolved into that water, what is the concentration of CO 2 ?

Question

While combusting in air, 4 g of H 2 gas was completely converted into water. If 36 μ mole of CO 2 from air is dissolved into that water, what is the concentration of CO 2 ? (A) 1 μ M (B) 1 mM (C) 1 nM (D) 1000 mM

Tardigrade Admin · Accepted Answer

The equation takes place as follows: underset4g2 H 2+ O 2 longrightarrow underset3 g 2 H 2 O ∵ 36 g of CO 2 is dissolved in 36 g of H 2 O. ∴ Conc. of CO 2 =(36 × 10-6 × 103/36) (∵ textconc. (C)=(n/V)) =10-3 M =1 mM

Q. While combusting in air, $4 g$ of $H_{2}$ gas was completely converted into water. If $36 μ$ mole of $C O_{2}$ from air is dissolved into that water, what is the concentration of $C O_{2}$ ?

$1 μ M$

$1 m M$

$1 n M$

$1000 m M$

The equation takes place as follows:

$4 g 2 H_{2} + O_{2} ⟶ 3 g 2 H_{2} O$

$∵ 36 g$ of $C O_{2}$ is dissolved in $36 g$ of $H_{2} O$ .

$∴$ Conc. of $C O_{2} = \frac{36 \times 1 0 ^{- 6} \times 1 0 ^{3}}{36}$

$(∵ conc. (C) = \frac{n}{V})$

$= 1 0^{- 3} M = 1 m M$

Q. While combusting in air, 4g of H2​ gas was completely converted into water. If 36μ mole of CO2​ from air is dissolved into that water, what is the concentration of CO2​ ?

1μM

1mM

1nM

1000mM