B is correct because both of the reactants are in ions form. So it does not have to undergo any bond break process, and accounts for its fastest reaction rate.
so to arrange them in decreasing order:
Can someone please answer the following question and in addition, name me the reactions from fastest to slowest and explain WHY things are the way they are? I got the answer when attempting it on my own but I feel it was just luck. The reason why I chose B was due to the charges making it an ionic bond but I don't know if this is WHY that answer is right. As for the other letters, I have absolutely no idea what to do with them (although the question doesn't ask for specifics, I'd like to know them please).
Based on the number and type of bonds to be broken and formed, which of the following chemical reactions would you expect to occur at the fastest rate at room temperature?
A) CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
B) Ag+(aq) + F-(aq)→ AgF(s)
C) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
D) Fe(s) + S(s) → FeS(s)
Any help would be GREATLY appreciated!
Thanks in advance!
Well, did you ask your teacher why the order is like this?
Anway, this is what i have learnt so far.
During chemical reactions, chemical bonds are broken and new bonds are formed. The nature (or type) of these chemical bonds and how readily they are broken and formed determines the rate of a reaction. When the reaction involves primarily the exchange of electrons (like the answer b), reactions tend to be very rapid. The phase of the reacting particles is important. Reactants in solution, liquids, and gases will react much faster than solids. Reactions involving covalently-bonded molecules tend to be slow unless highly exothermic