You double the partial pressure of a gas over a liquid at constant temperature. Which of these statements is then true? a. The Henry’s Law constant is decreased by half. b. There are half as many gas molecules in the liquid. c. There is no change in the number of gas molecules in the liquid. d. The Henry’s Law constant is doubled. e. There are twice as many gas molecules in the liquid.

Option (e) is the correct answer.

Explanation:

According to Henry's Law, mass of a gas which will dissolve into a solution is directly proportional to the partial pressure of that gas above the solution.

Mathematically,   C =

where,   = Henry's constant

               P = partial pressure

Since, concentration is directly proportional to partial pressure of a gas. Hence, more is the partial pressure more will be the number of molecules present in the liquid.

Thus, we can conclude that the statement there are twice as many gas molecules in the liquid, is true.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

elements make up everything, and they combine to make compounds.

the answer is c