Question

At 25.0 °C the Henry's Law constant for sulfur hexafluoride (SP) gas in water is 2.4x 10 M/atm Calculate the mass in grams of SFo, gas that can be dissolved in S25. ml. of water at 25.0 C and a SF, partial pressure of 1.90 atm Be sure your answer has the correct number of significant digits.

Answer 1

Complete Question

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Answer:

The mass is
`m = 0.0349 \ g`

Step-by-step explanation:

From the question we are told that

The Henry's Law constant is
`k = 2.4 *10^(10) M/atm`

The volume of water is
`V = 525 \ ml = 0.525 \ L`

The partial pressure is
`P = 1.90 \ atm`

The temperature is
`T = 25 ^oC`

Henry's law is mathematically represented as

`C = P * k`

Where C is the concentration of sulfur hexafluoride(SP)

substituting value

`C = 1.90 * 2.4*10^(-4)`

`C = 4.56*10^(-4) \ M`

The number of moles of SP is mathematically represented as

`n = C * V`

substituting value

`n = 0.525 * 4.56*10^(-4)`

`n = 2.39 *10^(-4) \ moles`

The mass of SP that dissolved is

`m = n * Z`

Where Z is the molar mass of SP which has a constant value of

`Z = 146 g/mole`

So

`m = 2.394*10^(-4) * 146`

`m = 0.0349 \ g`