A helium filled ballon at sea level gas a volume of 2.1L at 0.998 atm and 36C if it is released and rises to an elevation where the pressure is 0.900 atm and the temperature is 28.c what will be the new volume of the ballon

                      2.268 L

Explanation:

              According to Ideal Gas Law, " The Volume of a given mass of gas is inversely proportional to the applied Pressure and directly proportional to applied temperature, ". Mathematically the initial and final states of gas are given as,

                                     P₁ V₁ / T₁ =  P₂ V₂ / T₂   (1)

Data Given;

                  P₁  =  0.998 atm

                  V₁  =  2.1 L

                  T₁  =  36 °C  =  309 K

                  P₂  =  0.90 atm

                  T₂  =  28 °C  =  301 K

                  V₂  =  ??

Solving equation 1 for P₂,

                   V₂  =  P₁ V₁ T₂ / T₁ P₂

Putting values,

                   V₂  =  (0.998 atm × 2.1 L × 301 K) ÷ (309 K × 0.90 atm)

                   V₂  =  2.268 L

idk i’m struggling too