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

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

it takes on an electronical energy