2. A gas has a solubility in water
at 0°C of 3.6 g/L at a pressure
of 1.0 atm. What pressure is
needed to produce an aqueous
solution containing 9.5 g/L of
the same gas at 0°C?

2.6 atm

Explanation:

At constant temperature, solubility of gas increases as pressure increases, Hence, they varies directly proportional.

i.e  S ∝ P

where:

S₁ and P₁  are the initial solubility and pressure of the gas

S₂ and P₂ are the final solubility and pressure of the gas

Making P₂ the subject of the formula from the above equation; we have:

where; it is given from the question that:

P₁  = 1.0 atm

S₁ = 0.36 g/L

S₂ = 9.5 g/L

Replacing the values into the above equation; we have:

P₂ = 2.6 atm

∴  The pressure needed to produce an aqueous  solution containing 9.5 g/L of  the same gas at 0°C = 2.6 atm

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

the answer is minerals.