The Henry's law constant for CO2(g) in water at 25 °C is 29.4 bar·M–1. Estimate the concentration of dissolved CO2(g) in a carbonated soft drink pressurized with 1.95 bar of CO2(g).

Henry's Law says:


Pressure(gas)=(Henry's Law Constant)(Molarity of the gas)… we are looking for Molarity so we can rewrite the above equation as…

Molarity of the gas=Pressure(gas)/(Henry's Law Constant)
so… M=1.95 bar/29.4 barM-1

the bar units cancel when we divide giving the concentration of the gas in Molarity to be… 0.0663 M

YAY! hope this helps :)

Well, before I give you an answer, I have to warn you that estimating the concentration of dissolved CO2 in a carbonated soft drink can be as challenging as trying to find the elusive last potato chip in a bag. But fear not, because here's a way to estimate it using Henry's law constant.

According to Henry's law, the concentration of dissolved CO2 is directly proportional to the partial pressure of CO2. So, if we have a pressurized soft drink with 1.95 bar of CO2, we can use Henry's law constant to estimate the concentration.

Using the formula: Concentration = Henry's law constant × Partial pressure

Concentration = 29.4 bar·M⁻¹ × 1.95 bar

But hold your soda, because we need to convert units. The Henry's law constant is in bar·M⁻¹, and the partial pressure is also in bar. So, the units cancel out nicely:

Concentration = 29.4 M⁻¹ × 1.95

And after crunching some numbers, we get:

Concentration ≈ 57.33 M

So, the estimated concentration of dissolved CO2 in your pressurized carbonated soft drink is approximately 57.33 M. Just be careful not to drown in all that science while enjoying your fizzy drink!

To estimate the concentration of dissolved CO2(g) in the carbonated soft drink, we can use Henry's Law equation. The equation is given by:

C = k * P

Where:
C = Concentration of dissolved gas in solution (in Molarity)
k = Henry's Law constant (in bar·M–1)
P = Partial pressure of the gas above the solution (in bar)

In this case, the partial pressure of CO2(g) is 1.95 bar and the Henry's Law constant for CO2(g) in water at 25 °C is 29.4 bar·M–1.

Plugging in the values:

C = 29.4 bar·M–1 * 1.95 bar

C = 57.33 M

The estimated concentration of dissolved CO2(g) in the carbonated soft drink is 57.33 M.

To estimate the concentration of dissolved CO2 in a carbonated soft drink pressurized with 1.95 bar of CO2, we can use Henry's law, which states that the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of the gas.

Henry's Law equation is given as:

C = k * P

Where:
C is the concentration of the dissolved gas in the liquid
k is the Henry's law constant
P is the partial pressure of the gas

In this case, we are given the Henry's law constant for CO2 in water, k = 29.4 bar·M–1, and the partial pressure of CO2, P = 1.95 bar.

We can substitute these values into the equation to calculate the concentration:

C = 29.4 bar·M–1 * 1.95 bar

Performing the calculation:

C ≈ 57.33 M

Therefore, the estimated concentration of dissolved CO2 in the carbonated soft drink is approximately 57.33 M.

p = KC

1.85 = 29.4C
Solve for C.