Hydrogen, H2(g), is above silver metal in the activity series of the metals. WIll the follwing reaction, Ag(s) + H+(aq) -> occur or not occur? why or why not?
It will not.
A metal will displace any ion BELOW it in the activity series. Ag is BELOW H^+; therefore, it will not displace H^+
Thank you! I wasn't sure where H^+ was on the activity series
It's easy enough to find on google.
http://www.files.chem.vt.edu/RVGS/ACT/notes/activity_series.html
To determine whether the reaction Ag(s) + H+(aq) → will occur or not, we need to consider the position of hydrogen (H2) and silver (Ag) in the activity series of metals.
The activity series of metals lists metals in order of their reactivity. A metal located higher in the activity series is more reactive than a metal located lower in the series. Therefore, if hydrogen is higher than silver in the activity series, it indicates that hydrogen is more reactive than silver.
In this case, since hydrogen (H2) is above silver (Ag) in the activity series of metals, it means that hydrogen is more reactive than silver. As a result, hydrogen can displace silver from its compound. Hence, the reaction Ag(s) + H+(aq) → will occur.
However, it's important to note that this reaction will not produce hydrogen gas (H2(g)) as mentioned in the question. Instead, the hydrogen ion (H+) from the acid will react with silver metal (Ag(s)) to form silver ions (Ag+).
The balanced equation for the reaction can be represented as follows:
2Ag(s) + 2H+(aq) → 2Ag+(aq) + H2(g)
In summary, the reaction Ag(s) + H+(aq) → will occur because hydrogen is more reactive than silver, according to the activity series of metals.