To increase the solubility of a gas at constant temperature from 1.20 g/L at 1.4 atm to 2.3 g/L what would the pressure have to be increased to?
Its 2.7 thanks so much!
Henry's Law is p = kC
First, evaluate k from the first set of data. 1.2 atm = k(1.2g/L), then use k in the second set of p = kc to determine p. I found p to be about 2.5 or so but you need to confirm that and do it more accurately.
To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to _____.
To increase the solubility of a gas at constant temperature from 1.20 g/L, at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to _____.
To determine the pressure required to increase the solubility of a gas, 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.
Henry's Law equation: C = k * P
Where:
C = solubility of the gas in the liquid (in this case, in g/L)
k = Henry's Law constant for the specific gas-solvent combination
P = partial pressure of the gas above the liquid
In this case, we are given the initial solubility at a pressure of 1.4 atm (1.20 g/L), and we want to find the pressure required to increase the solubility to 2.3 g/L while keeping the temperature constant.
First, we need to determine the Henry's Law constant, which is specific to the gas-solvent combination. Once we have the constant, we can rearrange the equation to solve for the pressure.
Since we are not provided with the Henry's Law constant, we cannot directly calculate the pressure needed to achieve a solubility of 2.3 g/L.