A sample of gas initially occupies 2.50 L at a pressure of 0.900 atm at 22.0°C. What will the pressure be if the temperature is changed to 56.5°C, and the volume is changed to 1.50 L?

Final Pressure of the gas is 1.675 atm

Explanation:

Given: Initial Volume: V₁ = 2.5 L, Initial Pressure: P₁ = 0.9 atm, Initial Temperature: T₁ = 22 °C = 22 + 273 = 295 K

Final Volume: V₂ = 1.5 L, Final Temperature: T₂ = 56.5 °C = 56.5 + 273 = 329.5 K,                               (∵ 0°C = 273 K)

Final Pressure: P₂ = ?  

According to the Combined Gas Law:

Therefore, the Final Pressure of the given gas: P₂ = 1.675 atm

b. acid is the correct answer @jayxboof all social media

acid : acids are those which accepts an electron-pairs.

base : bases are those which donates ab electron-pairs.

alkali : it is a base that dissolves in water. it is basically a base and the ph greater than 7.

hydroxide ion : it is a poly-atomic ion which is negatively charged.