Question

ve
The Henry's law constant of a gas is 6.7x10-4 mol/(L bar). Its solubility when the partial pressure of the gas
at 298K is 0.65 bar is
(a) 4.355x104 mol/L
(b) 2.225x10 mol/L
(c) 4.355x102 mol/L
(d) 2.225x10 mol/L

Answer 1

Answer:

Correct Option is A

Hope help this answer

Answer 2

The correct option regarding the solubility of a gas is (a)

$4.355 \times {10}^{ - 4} \: mol /(L )$

Given:

Henry's law constant of gas is

$6.7 \times {10}^{ - 4} \: mol /(L bar)$ and partial pressure is 0.65 bar.

To Find:

The solubility.

Solution:

To find the solubility we will follow the following steps:

As we know,

When a gas dissolved in a liquid then the solubility is given by Henry's law:

$S \: = K× P$

Now,

According to the question:

$k = 6.7 \times {10}^{ - 4} \: mol /(L bar)$

$p = 0.65 \: bar$

Now,

In putting values we get,

$s = 6.7 \times {10}^{ - 4} \: mol /(L bar) \times 0.65 \: bar = 4.355 \times {10}^{ - 4} \: mol /(L )$

Henceforth, the correct option regarding the solubility of a gas is (a)

$4.355 \times {10}^{ - 4} \: mol /(L )$

#SPJ3