Henry’s law constant for CO2 is 1648atm at 298K. Calculate the number of moles of CO2 presentin 500ml of soda water, when packed under 2.5 atm CO2 pressure at 298K

To solve this problem, we will use Henry's Law, which states that the amount of dissolved gas is directly proportional to its partial pressure in the gas phase. The formula for Henry's Law is:

C = P/kH

where: C is the concentration of the dissolved gas, P is the partial pressure of the gas, kH is the Henry's Law constant.

Given: P = 2.5 atm, kH = 1648 atm, V = 500 ml = 0.5 L (since 1L = 1000ml)

We need to find C, the concentration of CO2 in moles/L.

Step 1: Substitute the given values into the Henry's Law formula:

C = P/kH C = 2.5 atm / 1648 atm C = 0.001517 L atm/mol

This is the concentration of CO2 in the soda water in terms of L atm/mol.

Step 2: Convert this concentration into moles/L.

We know that 1 L atm = 0.0821 mol (This is a constant known as the ideal gas constant)

So, C = 0.001517 L atm/mol * 0.0821 mol C = 0.000124 moles/L

Step 3: Multiply the concentration by the volume to get the number of moles of CO2:

n = C * V n = 0.000124 moles/L * 0.5 L n = 0.000062 moles

So, there are 0.000062 moles of CO2 present in 500 ml of soda water when packed under 2.5 atm CO2 pressure at 298K.