Given the following list from the activity se-
ries of metals (from most active to least ac-
tive)
K, Na, Al, Mn, Cr, Cd, Co, Pb, Hg
which reaction would you NOT expect to oc-
cur?
1. Na(s) +Mn2+(aq) ! Na+(aq) +Mn(s)
2. Co2+(aq) + Al(s) ! Al3+(aq) + Co(s)
3. Cd(s) + Pb2+(aq) ! Pb(s) + Cd2+(aq)
4. Al3+(aq) + Cr(s) ! Cr3+(aq) + Al(s)
5. All of the listed reactions will occur.
wouldn't it be 4 because those are both in the activity series under the category that displaces H from steam?
Metals will displace any ion below it in the activity series. For example, #1 will occur since Na (the metal) is above the Mn(ion).
it's 4
ut
To determine which reaction would NOT occur, we need to compare the activity of the metals involved in each reaction with the activity series of metals given.
The activity series of metals lists metals from most active (reactive) to least active (reactive). In this case, the list is:
K > Na > Al > Mn > Cr > Cd > Co > Pb > Hg
Now, let's analyze each reaction:
1. Na(s) + Mn2+(aq) → Na+(aq) + Mn(s)
In this reaction, Na is more active than Mn according to the activity series. Since more active metals can displace less active metals from their compounds, this reaction is expected to occur.
2. Co2+(aq) + Al(s) → Al3+(aq) + Co(s)
Comparing Al and Co, Al is more active than Co. Therefore, this reaction is also expected to occur.
3. Cd(s) + Pb2+(aq) → Pb(s) + Cd2+(aq)
Both Cd and Pb appear in the list of metals given. Cd is more active than Pb. Therefore, this reaction is expected to occur.
4. Al3+(aq) + Cr(s) → Cr3+(aq) + Al(s)
In this reaction, Al is more active than Cr according to the activity series. Hence, this reaction is also expected to occur.
Based on the information provided, all of the listed reactions should occur because the metals involved in each reaction are less active than the metals they are displacing. Therefore, the correct answer is:
5. All of the listed reactions will occur.