At 25 degrees C and 1 atm gas pressure, the solubility of CO2(g) is 149 mg/100 g water. When air at 25 degrees C and 1 atm is in equilibrium with water, what is the concentration of dissolved CO2, in mg/100 g water? Air contains 0.037 mol % CO2(g).

the answer should come out to be 5.5 x 10^-2 mg CO2/100 g H2O

Well, that's quite a mouthful of information! Let me see if I can sprinkle some humor into this scientific equation for you.

Ah, equilibrium, the magic dance of gases and liquids! Now, let's tackle this question step by step.

First, we have to convert the 0.037 mol % CO2 in air into an actual value. Remember, mol % is like a fancy way of saying "out of a hundred." So, if air contains 0.037 mol % of CO2, it means there are 0.037 moles of CO2 in every 100 moles of air. Phew, lots of numbers!

Now, the solubility of CO2 at 25 degrees C and 1 atm is given as 149 mg/100 g water. So, it means that 149 mg of CO2 will dissolve in every 100 g of water at those conditions. Hang in there, we're almost done!

To find the concentration of dissolved CO2 in mg/100 g water, we need to multiply the solubility (149 mg/100 g water) by the mol % of CO2 in air (0.037 mol %). Don't worry, I won't leave you to do the math.

So, multiplying 149 mg/100 g water by 0.037 mol %, we get approximately 5.5 x 10^-2 mg CO2/100 g H2O. Ta-da!

There you have it, my friend! The final answer is a hilarious 5.5 x 10^-2 mg CO2/100 g H2O. Remember, laughter is the best scientific solvent!

To find the concentration of dissolved CO2 in the water, we can use Henry's Law, which states that the concentration of a gas dissolved in a liquid is proportional to the partial pressure of the gas above the liquid.

Step 1: Convert air's CO2 concentration from mol % to partial pressure
Given that air contains 0.037 mol % CO2, we can calculate the partial pressure of CO2 using the ideal gas law:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.

At 25 degrees C and 1 atm, the partial pressure of CO2 can be calculated as follows:
0.037 mol % = 0.037/100 = 0.00037 (mol CO2/mol air)
Partial pressure of CO2 in air = 0.00037 * 1 atm = 0.00037 atm

Step 2: Use Henry's Law to calculate the concentration of dissolved CO2
Henry's Law is given by:
C = k * P
where C is the concentration of dissolved CO2, P is the partial pressure of CO2, and k is the Henry's Law constant.

Given that the solubility of CO2 at 25 degrees C and 1 atm is 149 mg/100 g water, we can rearrange the equation to solve for k:
149 mg/100 g = k * 1 atm

k = (149 mg/100 g) / (1 atm) = 1.49 mg/(100 g * atm)

Now we can substitute the values into the Henry's Law equation:
C = (1.49 mg/(100 g * atm)) * (0.00037 atm)
C = 5.513 x 10^-4 mg/100 g

Therefore, the concentration of dissolved CO2 in the water will be approximately 5.5 x 10^-4 mg/100 g, which is approximately 5.5 x 10^-2 mg CO2/100 g H2O.

To find the concentration of dissolved CO2 in mg/100 g water, we need to use the given solubility of CO2 and the mole percent of CO2 in air.

Step 1: Convert the mole percent of CO2 to mol/mol air:
0.037 mol % CO2 means that for every 100 mol of air, there are 0.037 mol of CO2.

Step 2: Convert mol/mol air to mol/L of solution:
Since the concentration is usually expressed in mg/100 g water, we need to convert mol/mol air to mol/L of solution first.
Assuming that the density of air is approximately 1 g/L, the mole percent of CO2 can be converted to mol/L as follows:
0.037 mol CO2 / (100 mol air/L) = 0.00037 mol CO2 / L of solution

Step 3: Use the solubility of CO2 to convert to mg/100 g water:
The solubility of CO2 is given as 149 mg CO2 / 100 g water.
Since we need the concentration in mg/100 g water, we divide the solubility by 100 g water:
149 mg CO2 / (100 g water) = 1.49 mg CO2 / g water

Step 4: Multiply the solubility by the concentration of CO2 in mol/L:
To find the concentration of CO2 in mg/100 g water, we multiply the solubility by the concentration in mol/L:
1.49 mg CO2 / g water * 0.00037 mol CO2 / L = 0.00055013 mg CO2 / g water

Step 5: Convert mg/g water to mg/100 g water:
The remaining value is in mg CO2/g water, so we multiply it by 100 to get the concentration in mg/100 g water:
0.00055013 mg CO2 / g water * 100 = 0.055013 mg CO2 / 100 g water

Rounding off the result to the appropriate number of significant figures, the concentration of dissolved CO2 in mg/100 g water is approximately 5.5 x 10^-2 mg CO2/100 g H2O.

(149 mg/100) x 0.00037 = ?