Question

use the activity series below to predict the products of each of the following reactions. you do not need to balance the equations.
li > k > ba > sr > ca > na > mg > al > mn > zn > cr > fe > cd >
co > ni > sn > pb > h > sb > bi > cu > ag > pd > hg > pt > au
f₂ > cl₂ > br₂ > i₂
ccl₄ + br₂ → ?
☑ no reaction
brcl + c
cbr₄ + cl₂
complete
feso₄ + na → ?
○ no reaction
○ na₂so₄ + fe
○ fena + so₄
done

Explanation:

For the reaction $\boldsymbol{\ce{CCl4 + Br2 ->}}$:

Step1: Check halogen activity series

The halogen activity series is $\ce{F2 > Cl2 > Br2 > I2}$. This means a halogen can displace another halogen from its compound only if it is more reactive (higher in the series).

Step2: Compare $\ce{Br2}$ and $\ce{Cl2}$ reactivity

Here, we are looking at the reaction between $\ce{CCl4}$ (containing $\ce{Cl}$) and $\ce{Br2}$. Since $\ce{Br2}$ is less reactive than $\ce{Cl2}$ (because $\ce{Cl2}$ is higher in the halogen activity series than $\ce{Br2}$), $\ce{Br2}$ cannot displace $\ce{Cl}$ from $\ce{CCl4}$. So, there is no reaction.

For the reaction $\boldsymbol{\ce{FeSO4 + Na ->}}$:

Step1: Check metal activity series

The metal activity series is $\ce{Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb > H > Sb > Bi > Cu > Ag > Pd > Hg > Pt > Au}$.

Step2: Compare $\ce{Na}$ and $\ce{Fe}$ reactivity

Sodium ($\ce{Na}$) is more reactive than iron ($\ce{Fe}$) because $\ce{Na}$ is higher in the metal activity series than $\ce{Fe}$. In a single - displacement reaction, a more reactive metal can displace a less reactive metal from its salt solution. So, $\ce{Na}$ will displace $\ce{Fe}$ from $\ce{FeSO4}$. The reaction will be $\ce{FeSO4 + Na -> Na2SO4 + Fe}$ (we don't need to balance it here).

Answer:

s:

• For $\ce{CCl4 + Br2 ->}$: no reaction
• For $\ce{FeSO4 + Na ->}$: $\ce{Na2SO4 + Fe}$ (the option is: $\boldsymbol{\ce{Na2SO4 + Fe}}$)