Question

The value of carbon monoxide gas collected
over water at 25°C is 680 cc. with a total pressure of 752 mm
Hg. The vapour pressure of water at 25°C is 23.8 mm Hg.
Determine the partial pressure of CO in container.​

Answer 1

Answer:

From the basic law of Dalton law of partial pressure P=p1+p2

Explanation:

Please send me the answer I want make sure myself that I am correct

Answer 2

Final answer: Partial pressure of $CO$ in container = 728.2 mm Hg

Given that: We are given,

  (i) Total pressure = 752 mm Hg

  (II) Vapour pressure of water at 25°C = 23.8 mm Hg

To find: We have to find partial pressure of $CO$ in container.

Explanation:

• In accordance with the Dalton's  partial pressure law, total pressure exerted by a mixture of gases is the sum of the partial pressures exerted by individual gases in that mixture.

i.e. $P_{total} = p_{1} + p_{2} + ... + p_{n}$

$P_{total}$ = Total pressure

$p_{1} + p_{2} + ... + p_{n}$ = Partial pressures of the gases 1, 2,…,n

• Here, mixture contain carbon monoxide-$CO$ and water-$H_{2}O$.

$P_{total} = p_{CO} + p_{H_{2}O}$

• Given that vapour pressure of water at 25 °C is 23.8 mm Hg.

$p_{H_{2}O}$ = 23.8 mm Hg

Total pressure, $P_{total}$  = 752 mm Hg

• $p_{CO}$ = ?

Substitute the values of  $P_{total}$, $p_{H_{2}O}$:

$752 mm Hg = p_{CO}+ 23.8 mm Hg$

$p_{CO}= 752 mm Hg - 23.8 mm Hg$

$p_{CO}= 728.2 mm Hg$

• Hence, partial pressure of $CO$ in container = 728.2 mm Hg

To know more about the concept please go through the links

https://brainly.in/question/14872724

https://brainly.in/question/5362246

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