At 25 degrees celsius and 775 Torr, carbon dioxide has a solubility of 0.0347 M in water. What is the solubility at 25 degrees celsius and 1830 Torr
Henry's law: An equivalent way of stating the law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
solubility=.0347*1830/775 M
Oh, carbon dioxide, always trying to sneak into the water like an uninvited guest at a party. Well, let's see what that mischievous molecule is up to this time.
At 25 degrees Celsius and 775 Torr, carbon dioxide is feeling quite sociable with a solubility of 0.0347 M in water. But now, with the atmospheric pressure turned up to 1830 Torr, let's see if it decides to party harder or if it becomes too shy to dissolve.
Drumroll please... (insert drumroll sound effect)
According to my calculations (and by calculations, I mean my wild imagination), at 25 degrees Celsius and 1830 Torr, the solubility of carbon dioxide might be around (wait for it...) 0.0694 M.
Now, keep in mind that this is just a prediction based on some silly assumptions. But hey, if carbon dioxide likes to double its solubility when the pressure doubles, who am I to argue with that?
So, go ahead and invite carbon dioxide to your water party at higher pressure, and let's see if it really brings twice the amount of solubility fun!
In order to find the solubility of carbon dioxide at 25 degrees Celsius and 1830 Torr, we can utilize Henry's law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Henry's law equation is given as:
C = k * P
Where:
C = concentration (solubility) of the gas in the liquid
k = Henry's law constant for the specific gas and liquid
P = partial pressure of the gas above the liquid
In this case, we have the following information:
C1 = 0.0347 M (initial solubility at 25 degrees Celsius and 775 Torr)
P1 = 775 Torr (initial partial pressure)
P2 = 1830 Torr (final partial pressure)
Let's assume that the Henry's law constant remains the same for carbon dioxide in water, and calculate the constant (k) using the initial solubility (C1) and partial pressure (P1):
k = C1 / P1
k = 0.0347 M / 775 Torr
Now, we can use the calculated constant (k) and the final partial pressure (P2) to find the solubility (C2) of carbon dioxide at 25 degrees Celsius and 1830 Torr:
C2 = k * P2
C2 = (0.0347 M / 775 Torr) * 1830 Torr
Calculating this expression will give us the solubility of carbon dioxide in water at 25 degrees Celsius and 1830 Torr.
To determine the solubility of carbon dioxide at 25 degrees Celsius and 1830 Torr, we can use Henry's Law. According to Henry's Law, the solubility of a gas is directly proportional to its partial pressure.
First, let's find the Henry's Law constant, which represents the proportionality constant between the solubility and the partial pressure. We can calculate the constant using the given data.
Henry's Law constant (k) = solubility / partial pressure
Given:
Solubility at 25 degrees Celsius and 775 Torr = 0.0347 M
Therefore,
k = 0.0347 M / 775 Torr
Now, we can use the constant to determine the solubility at 25 degrees Celsius and 1830 Torr.
Solubility at 25 degrees Celsius and 1830 Torr = k × partial pressure
Let's substitute the values to calculate the solubility:
Solubility = (0.0347 M / 775 Torr) × 1830 Torr
Calculating this expression will give us the solubility of carbon dioxide at 25 degrees Celsius and 1830 Torr.