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 $m = 0.0349 \ g$

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

         $m = 2.394*10^{-4} * 146$

         $m = 0.0349 \ g$