A sample of Br2 gas has a volume of 29.0L and a pressure of 1.50 atm. If the initial temperature of the gas is 23 °C, what volume, in liters, will the gas occupy at 3.50 atm and 271 °C?

V₂ = 22.84 L

Explanation:

Given data:

Initial volume = 20.0 L

Initial pressure = 1.50 atm

Initial temperature = 23 °C (23 +273 = 296 K)

Final temperature = 271°C (271+273 = 544 K)

Final pressure = 3.50 atm

Final volume = ?

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

V₁ = Initial volume

T₁ = Initial temperature

P₂ = Final pressure

V₂ = Final volume

T₂ = Final temperature

Solution:

V₂ = P₁V₁ T₂/ T₁ P₂  

V₂ = 1.50 atm × 29.0L ×544 K / 296 K × 3.50 atm

V₂ = 23664 atm .L. K / 1036 atm.K

V₂ = 22.84 L

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.