Assign oxidation numbers to each of the elements in this unbalanced redox reaction. Cl2(g)+I^-(aq)--->Cl^-(aq)+IO3^-(aq)
Assign oxidation states to all the elements in this unbalanced reaction: Ag+(aq) + Cu(s) --> Ag(s) + Cu2+ (aq) Which substance gets oxidized? Which substance gets reduced? Balance the Redox reaction.
Redox. For each reaction below: 1) Ensure that the reaction is balanced. 2) Assign oxidation numbers to each reactant and product 3) Identify which atom was oxidized and which atom was reduced. 4) Identity which atom is the oxidizing agent, and which is the reducing agent A) Br2(l)+I^-(aq) --->Br^-(aq)+I2(s) B)Cr2O7^2-(aq)+Fe^2+(aq)--->Cr^3+(aq)+Fe^3+(aq) C) NO3^-(aq)+I2(aq)--->IO3^-(aq)+NO2(aq)
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Assign oxidation states to al the elements In this unbalanced reaction: Ag^+(aq) + Cu(s) rightarrow Ag(s) + Cu^2+ (aq) Which substance gets oxidized? Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq) Which substance gets reduced? Balance the redox reaction: Ag^+(aq) Cu(s) Ag(s) Cu^2+(aq)
Assign the correct oxidation number to each species in the redox reaction below. PbSO4(s) + H*(aq) + 2Cl(aq) = Pb(s) + H$04" (aq) + Cl2(g)
Identify the species (atoms/ elements) undergoing oxidation and
reduction in the following equations, assign oxidation numbers to
each, and write balanced net ionic equations.
a) Cu(s)
Cu2+(aq) + 2e-
b) Cl2(aq) + 2e-
Cl-(aq)
c) Cu(s) + Cl2(aq)
Cu2+(aq) + 2Cl-(aq)
d) 4CuO(s) + CH4(g)
4Cu(s) + CO2(g) + 2H2O(l)
e) 2CuSO4(aq) + 4KI(aq)
2CuI (aq) + 2K2SO4(aq) +
I2(aq)
f) Cu2O(s) + Fe(SO4)3 (aq) +
H2SO4(aq)
2CuSO4(aq) + 2FeSO4(aq) +
H2O(l)
Oxidation Numbers 1. Assign oxidation numbers to the atoms in each of the following. a) SO2 d) Mgl b) HCIO e) CaH c) Cr,0,2 f) Fe, 2. For each of the following: •assign oxidation numbers •indicate whether the equation represents a redox reaction .if redox, identify OA and RA a) Cu + 2 AgNO, 2 Ag + Cu(NO3)2 b) Pb(NO3)2 + 2 KI Pbl, + 2 KNO, c) Cl2 + 2 KI I2 + 2 KCI d) 2 NaCl 2...
Under acidic conditions, the iodide ion is oxidized by the iodate ion in the presence of excess chloride to form the compound iodine chloride according to the following unbalanced reaction. IO3−(aq) + I−(aq) + Cl−(aq)→ICl(aq) a) Determine the oxidation numbers for each atom. b) Balance the equation.
For the following reaction, (1) assign oxidation numbers for all the elements, (2) determine which one is oxidized and which one is reduced, and (3) balance the redox reaction in acidic solution. SO32–(aq) + MnO4–(aq) ® SO42–(aq) + Mn2+(aq)
Balance the following redox reaction in basic solution. Cl (aq)+Cro (aq) - Cl2(g)+Cr(OH)3(s) Cl (aq) Cro (aq) C,(g) Cr(OH), (s)
Use the half-reaction method to balance each redox reaction occurring in acidic aqueous solution. Cl−(aq)+MnO4−(aq)→Cl2(g)+Mn2+(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.