A sample of argon has a volume of 5.0 dm^3 and the pressure is 0.92 atm.
If the final temperature is 30.° C, the final volume is 5.7 L, and the final
pressure is 800. mm Hg, what was the initial temperature of the argon?

232.9K

Explanation:

V₁  = 5dm³

P₁  = 0.92atm

T₂ = 30°C

V₂ = 5.7L

P₂ = 800mmHg

Unknown:

T₁ = ?

Solution:

To solve this problem, we are going to apply the combined gas law which is fusion of the avogadro's law, boyle's law and charles's law.

 Mathematically;

p, v and T are pressure, volume and temperature respetively

1 and 2 depicts the initial and final states.

We need to convert ;

     temperature to K and pressure into atm

T₂  = 30°C  = 273 + 30 = 303K

P₂  =  800mmHg;

         760mmHg  = 1 atm

           800mmHg  =  = 1.05atm

   Input the variables and solve;

    T  = 232.9K

i would say b

explanation:

but i think i would need more information than that