A gas expands from a volume 2.0 L at 36oC to a volume of 2.5 L, what is the final temperature, if the pressure is constant?

386.45 K

Explanation:

We can solve this problem by using Charles' law, which states that at constant pressure:

V₁T₂=V₂T₁

Where subscript 1 stands for initial conditions of volume and temperature, while 2 stands for the final ones. Meaning that in this case:

V₁ = 2.0 LT₂ = ?V₂ = 2.5 LT₁ = 36 °C ⇒ 36 +273.16 = 309.16 K

We input the data:

2.0 L * T₂ = 2.5 L * 309.16 K

And solve for T₂:

T₂ = 386.45 K

The activity series is shown in the attached picture. if the element is below the other, then you can displace the other. following the activity series as a guide, the reactions are as follows: nickel and aluminum chloride3 ni + 2 alcl₃  → 3 nicl₂ + 2 albarium and copper bromideba + cubr  →  no reaction because cu is less oxidizable than bapotassium nitrate and aluminum3 kno₃ + al  → al(no₃)₃ + 3 ksodium phosphate and zincnaso₄ + zn  → znso₄ + na