A350 ml sample of gas has a temperature of 30°c and a pressure of 1.20 atm. what temperature
would be needed for the same amount of gas to fit into a 250 ml flask at standard pressure?

T₂ = 180.4 K

Explanation:

According to general gas equation:

P₁V₁/T₁ = P₂V₂/T₂

Given data:

Initial volume = 350 mL

Initial pressure = 1.20 atm

Initial temperature = 30 °C (30 +273 = 303 K)

Final volume = 250 mL

Final pressure = 1 atm

Final temperature = ?

Solution:

P₁V₁/T₁ = P₂V₂/T₂

T₂  =   P₂V₂ T₁ /P₁V₁

T₂ = 1 atm × 250 mL × 303 K / 1.20 atm × 350 mL

T₂ =  75750 atm .mL.  K  / 420 atm. mL

T₂ = 180.4 K

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.

i would say b

explanation:

but i think i would need more information than that