What is the mass of gas dissolved in a solution at 150kPa if 0.35g of the gas dissolves in 2.0L of water at 30kPa?
To find the mass of gas dissolved in a solution at 150 kPa, when 0.35 g of the gas dissolves in 2.0 L of water at 30 kPa, we can use the combined gas law.
The combined gas law equation is:
(P1 * V1) / T1 = (P2 * V2) / T2
Where:
P1 = initial pressure (30 kPa)
V1 = initial volume (2.0 L)
T1 = initial temperature (unknown)
P2 = final pressure (150 kPa)
V2 = final volume (unknown)
T2 = final temperature (unknown)
We know the initial and final pressures (P1 = 30 kPa and P2 = 150 kPa) and the initial volume (V1 = 2.0 L). Let's assume the temperature remains constant (T1 = T2).
The equation becomes:
(30 kPa * 2.0 L) / T = (150 kPa * V2) / T
To solve for V2, we rearrange the equation:
V2 = [(30 kPa * 2.0 L) / (150 kPa)] * T
Now, we need to find the final volume (V2) to determine the mass of the gas dissolved in the solution. However, since we don't have the final temperature (T), we are unable to calculate it at this point.
To find the mass of gas dissolved in a solution at a different pressure, we can use 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. According to Henry's law, we can set up a proportion to solve for the mass of gas at 150 kPa.
Let's define the variables:
m₁ = mass of gas dissolved at 30 kPa
P₁ = pressure at which the gas is dissolved (30 kPa)
m₂ = mass of gas dissolved at 150 kPa (what we want to find)
P₂ = pressure at which we want to find the mass of gas (150 kPa)
According to Henry's law, we can set up the following proportion:
(m₁ / P₁) = (m₂ / P₂)
Substituting the given values:
(0.35g / 30 kPa) = (m₂ / 150 kPa)
Now we can solve for m₂:
m₂ = (0.35g / 30 kPa) * 150 kPa
m₂ = (0.35g / 2) * 5
m₂ = 0.35g * 5 / 2
m₂ = 1.75g
Therefore, the mass of gas dissolved in the solution at 150 kPa is 1.75 grams.
I think,
(150kPa/30kPa)*0.35g= mass of gas dissolved in a solution at 150kPa
Not sure.