To increase the solubility of a gas at constant temperature from 1.20 g/L at 1.4atm to 2.3 g/L the pressure would have to be increased to ______
A. 0.37 atm
B. 0.7 atm
C. 1.37 atm
D. 2.7 atm
Hmmmm , well I have to know because its a take home quiz but thanks!
Use pressure = kc
Calculate k from the first set of data given and use the same k with different c to calculate new pressure. (I might point out that answer B is not an increase in pressure but a decrease. The problem asks what INCREASE...).
Oops. I spelled my name wrong. Anyways, the Buddha knows all. It is D.
To determine the pressure required to increase the solubility of a gas, we can use the relationship known as Henry's Law. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
The equation for Henry's Law is given as:
C = k * P
where C is the solubility of the gas in the liquid, P is the partial pressure of the gas, and k is the Henry's Law constant.
In this case, we are given the initial solubility (1.20 g/L) at a pressure of 1.4 atm, and we want to find the pressure required for the solubility to increase to 2.3 g/L.
We can set up a proportion using the solubility and pressure values:
1.20 g/L / 1.4 atm = 2.3 g/L / x atm
We can solve this equation for x (the unknown pressure) by cross-multiplying and dividing:
1.20 g/L * x atm = 2.3 g/L * 1.4 atm
x = (2.3 g/L * 1.4 atm) / 1.20 g/L
x = 3.22 atm / 1.20 g/L
x ≈ 2.6833 atm
Therefore, the pressure required to increase the solubility to 2.3 g/L is approximately 2.6833 atm. Rounded to one decimal place, the answer would be 2.7 atm.
Hence, the correct answer is D. 2.7 atm.