Why is a mixture of $He-O_2$ used by deep-sea divers instead of a $N_2-O_2$ mixture?
- AHelium is much less soluble in blood than nitrogen.
- BNitrogen is much less soluble in blood than helium.
- CAt high pressure in deep sea,nitrogen and oxygen react to form toxic nitric oxide.
- DNitrogen is highly soluble in water.
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Similar Questions
Identify from the following salts the one whose solubility in water decreases with an increase in temperature.
If $N_2$ gas is bubbled through water at $293 \ K$,how many millimoles of $N_2$ gas would dissolve in $1 \ L$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. The Henry's law constant for $N_2$ at $293 \ K$ is $76.48 \ kbar$.
Medium
View SolutionHenry's law constant for the molality of methane in benzene at $298 \, K$ is $4.27 \times 10^{5} \, mm \, Hg$. Calculate the solubility of methane in benzene at $298 \, K$ under $760 \, mm \, Hg$.
Easy
View SolutionHenry's constant (in $kbar$) for four gases $\alpha, \beta, \gamma$ and $\delta$ in water at $298 \ K$ is given below:
Gas $K_{H} \ (kbar)$ $\alpha$ $50$ $\beta$ $2$ $\gamma$ $2 \times 10^{-5}$ $\delta$ $0.5$
(Density of water $= 10^{3} \ kg \ m^{-3}$ at $298 \ K$). This table implies that:
| Gas | $K_{H} \ (kbar)$ |
| $\alpha$ | $50$ |
| $\beta$ | $2$ |
| $\gamma$ | $2 \times 10^{-5}$ |
| $\delta$ | $0.5$ |
(Density of water $= 10^{3} \ kg \ m^{-3}$ at $298 \ K$). This table implies that:
Calculate $K_H$ when $2 \ mmol$ of $O_2$ dissolve in $540 \ mL$ of water at $27 \ ^oC$ temperature. Given $P_{O_2} = 2 \times 10^{-8} \ bar$.
Medium
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