Which reaction is NOT a redox reaction?
CH4+2O2=CO2+2H2O
2Na+CI2=2NaCI
AgNO3+NaCI=AgCI+NaNO3
KCIO3=KCI+3/2O2
I chose, KCIO3=KCI+3/2O2. Is this correct?
Yes
absolutely not correct because:.
KClO3 ==> KCl + 3/2 O2
Cl on the left is +5 oxidation state and on the right it is -1 while
O on the leftr is -2 and on the right is zero. Loss and gains of electrons certainly is redox.
I second guessed myself. The original answer I had was CH4+2O2=CO2+2H2O. Is this correct Dr. Bob?
C'mon. The only way to do this problem is not to guess.
You go through and assign oxidation states to each element and the ones that don't change are not redox; those that do change are redox. For your second guess here are the numbers.
On the left C is -4, H is +1, O is zero.
On the right C is +4, H is +1, O is -2
So C and O changed. Must be redox. In chemistry one NEVER has to guess. You can figure all these things out one by one. I can give you a link if you don't know how to assign oxidation states.
Okay. I've done what you said and found that the oxidation numbers for AgNO3 + NaCI = AgCI + NaNO3 do not change. This must not be redox.
You are right. That is the only one listed that is NOT redox and that's what the problem wanted: i.e., the equation that was not redox.
Yes, you are correct. The reaction KCIO3 = KCI + 3/2O2 is not a redox reaction.
To determine whether a reaction is a redox reaction, you need to examine the changes in oxidation states of the elements involved.
In a redox reaction, there is a transfer of electrons from one species to another. This transfer leads to a change in the oxidation state (or oxidation number) of the elements. The species that loses electrons is being oxidized (oxidation state increases), while the species that gains electrons is being reduced (oxidation state decreases).
Let's analyze the reactions you provided:
1. CH4 + 2O2 = CO2 + 2H2O: In this reaction, carbon (C) in CH4 is oxidized from -4 to +4 in CO2, while oxygen (O) is reduced from 0 to -2 in CO2. Therefore, this is a redox reaction.
2. 2Na + Cl2 = 2NaCl: In this reaction, sodium (Na) loses an electron and is oxidized from 0 to +1 in NaCl, while chlorine (Cl) gains an electron and is reduced from 0 to -1 in NaCl. Therefore, this is a redox reaction.
3. AgNO3 + NaCl = AgCl + NaNO3: In this reaction, silver (Ag) changes from +1 to 0 in AgCl, while nitrogen (N) changes from +5 to +5 in NaNO3, and chlorine (Cl) changes from -1 to -1 in NaCl. Although there is a change in oxidation state for silver, there is no net transfer of electrons; therefore, this is not a redox reaction.
4. KCIO3 = KCI + 3/2O2: In this reaction, potassium (K) does not change its oxidation state (always +1), chlorine (Cl) does not change its oxidation state (always -1), and iodine (I) in KCIO3 changes from +5 to -1 in KCI. There is no transfer of electrons between any of the elements, so this is not a redox reaction.
Therefore, your choice of KCIO3 = KCI + 3/2O2 as the reaction that is not a redox reaction is correct.