Asample of he gas (v = 3.0 l) at 5.6 atm and 25 °c was combined with 4.5 l of ne gas at 3.6 atm and 25 °c in a 9.0 l flask (which was initially evacuated). what is the total pressure in the 9.0 l flask after mixing? assume the temperature remains at 25 °c.

3.67 atm

Explanation:

Because the gases are not reacting and the temperature remaining the same, we can apply Boyle's Law:

P1V1 = P2V2

Where P is the pressure, V is the volume, 1 is the initial state, and 2 the final state.

For a mixture of gases, from Dalton's law, the total pressure is the sum of the partial pressures of the components, so:

P1V1 = PHe*Ve + PNe*VNe

PHe*Ve + PNe*VNe = P2*V2

5.6*3.0 + 3.6*4.5 = P2*9

9P2 = 33

P2 = 3.67 atm

beta decay is the answer

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