Achemist prepares a solution of iron(ii) bromide febr2 by measuring out 0.55kg of iron(ii) bromide into a 500.ml volumetric flask and filling the flask to the mark with water.

calculate the concentration in /moll of the chemist's iron(ii) bromide solution.
round your answer to 2 significant digits

Molar mass of ferrous bromide: 215.65
m(FeBr2): 550/215.65 = 2.55moles
this is dissolved in 500mL of water so in 1L of solution there will be 2.55x2 = 5.1mol/L

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