At atmospheric pressure of 1 atm, the partial pressure of oxygen in air is 0.21 atm. At this atmospheric pressure and 25°C, water contains 2.73 x 10^-4 M dissolved oxygen gas. What is the Henry's Law constant for oxygen dissolved water at this temperature in terms of M and atm?
H = c/p = 2.73E-4/0.21 = ?
Well, I must say, trying to calculate Henry's Law constant using M and atm is like trying to catch a clown fish with a butterfly net – it can be quite tricky! But fear not, my friend, Clown Bot is here to provide some clownishly entertaining assistance!
To calculate Henry's Law constant (k) for oxygen dissolved in water, we need to use the equation:
C = k * P
Where C is the concentration of dissolved oxygen (in M), k is the Henry's Law constant (in M/atm), and P is the partial pressure of oxygen (in atm).
In your case, you're given that the partial pressure of oxygen in the air is 0.21 atm and the concentration of dissolved oxygen in water is 2.73 x 10^-4 M. So, we can rearrange the equation and solve for k:
k = C / P
Substituting the given values:
k = (2.73 x 10^-4 M) / (0.21 atm)
Now, let me punch in those numbers and calculate it for you...
*clownish sound effects*
Beep boop beep boop beep... Calculating...
And the answer, my friend, is approximately k = 1.3 x 10^-3 M/atm.
So, the Henry's Law constant for oxygen dissolved in water at this temperature is approximately 1.3 x 10^-3 M/atm.
I hope I was able to put a smile on your face with this nerdy clown act of mine! If you have any more questions, feel free to ask, and Clown Bot will be here to entertain you!
To find the Henry's Law constant (k), we can use the equation:
C = k * P
Where:
C = concentration of the dissolved gas in M (moles per liter)
k = Henry's Law constant
P = partial pressure of the gas in atm
Given values:
Partial pressure of oxygen (P) = 0.21 atm
Concentration of dissolved oxygen (C) = 2.73 x 10^-4 M
We can rearrange the equation to solve for k:
k = C / P
Substituting the given values:
k = (2.73 x 10^-4 M) / (0.21 atm)
k ≈ 1.3 x 10^-3 M/atm
Therefore, the Henry's Law constant for oxygen dissolved in water at this temperature is approximately 1.3 x 10^-3 M/atm.
Henry's Law relates the concentration of a gas dissolved in a solution to its partial pressure. It can be expressed using the equation:
C = k * P
where:
C is the concentration of the gas in the solution (in M),
k is the Henry's Law constant, and
P is the partial pressure of the gas (in atm).
To find the Henry's Law constant (k) for oxygen dissolved in water, we need to rearrange the equation to solve for k:
k = C / P
From the given information, we have:
C = 2.73 x 10^-4 M (concentration of dissolved oxygen in water)
P = 0.21 atm (partial pressure of oxygen in air)
Substituting these values into the equation, we can calculate the Henry's Law constant:
k = (2.73 x 10^-4 M) / (0.21 atm)
Calculating this expression, we get:
k = 1.30 x 10^-3 M/atm
Therefore, the Henry's Law constant for oxygen dissolved in water at this temperature (25°C) is approximately 1.30 x 10^-3 M/atm.