Redox Reactions?
A. H+(aq) + HS−(aq) → H2S(g)
B. Ni(OH)2(s) + 2HCl(aq) → NiCl2(aq) + 2H2O(l)
C. Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)
D. 2K(s) + I2(s) → 2KI(s)
E. Fe(s) + 2AgNO3(aq) → Fe(NO3)2(aq) + 2Ag(s)
I think its
A. Correct
B. Incorrect
C. Incorrect
D. Incorrect
E. Correct
Can someone tell me where I'm going wrong or help me please?
-Thanks in Advance
Answer:
you gotta have a look at the charges on the respective ions
H only redoxes to form H2, so C is a redox, also the Fe changes from 0 charge to 2+ charge
S doesn't change charge, so A is not
Ni doesn't change charge, so B is not
K goes from 0 charge to 1+ charge while I goes from 0 charge to 1-, so D is redox
Fe from 0 charge to 2+ and Ag from 1+ to 0 charge, E is redox
the oxidation mean loss of electron and reduction mean gain electron and it must be in SAM time , A H did not loss any electron and because S have empty orbitals it take another H atom and so on
A incorrect
B incorrect
C correct
D incorrect
E correct
and that what iam think about so plz check it again
i could be wrong.
The answers post by the user, for information only, FunQA.com does not guarantee the right.
More Questions and Answers: