a sample of methane gas at a pressure of 0.815 atm and a temperature of 265 C occupies a volume of 416 mL. If the gas is heated at constant pressure until its volume is 593 ml the temperature of the gas will be C

493.9°C

Explanation:

Given parameters:

Initial pressure  =0.815atm

Initial temperature  = 265C  = 265 + 273  = 538k

Initial volume  = 416mL  = 0.416L

New volume    = 593mL  = 0.593L

Unknown:

New temperature =?

Solution:

Since we are dealing with constant pressure condition, we apply charles's law.

It states that the volume of a fixed mass of gas varies directly as its absolute temperature if the pressure is constant.

    Mathematically ;

             =  

V1 is the initial volume                     V2 is the new volume

T1 is the initial temperature             T2 is the new temperature

      =    

           T2 = 766.9K;

  In °C  = 766.9 - 273 = 493.9°C

i'm assuming that it's c.) red bank..