Complete and balance the following redox reaction in basic solutio Zn(s) → Zn(OH),²(aq) + H,(g)

Consider the following net ionic equation: MnO,(aq) + s²- (aq) –→ MnO,(s) + S(s)

Write and balance a net ionic equation for each reaction and include states of matter. (a) NaCl + Ag2SO4→Na2SO4 + AgCl (b) Cu(OH)2 + HCl→CuCl2 + H2O (c) BaCl2 + Ag2SO4→BaSO4 + AgCl

Balance the following redox reaction under acidic conditions. H2O2(aq) + Cl2O7(aq)  =  ClO2-(aq) + O2(g)

Which reaction(s) can be identified as a redox reaction? CuO(s) + H₂SO4(aq) → CuSO4(aq) + H₂O(1) Cu(NO3)2(aq) + 2NaOH(aq) -> A →→ Cu(OH)₂(s) + 2NaNO3(aq) Cu(OH)2(s) CuO(s) + H₂O(g) CuSO4(aq) +Zn(s) → ZnSO4(aq) + Cu(s) Cu(s)+ 4HNO3(aq) - Cu(NO3)2(aq) + 2NO₂(aq) + 2H₂O(1)

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cl2 and OH- in the balanced reaction?Cl2(g) → ClO3-(aq) + Cl-(aq)

Predict the product and then balance the redox reaction. Identify which reagent acts as the oxidizer. Al (s) + HNO3 (aq) = ?

What element is being oxidized in the following redox reaction? MnO4 (aq) + H2C204laq) → Mn2*(ag) + CO2(g) Mn Oc

For the following (potentially unbalanced) reaction, determine what is being (a) reduced and (b) oxidized, (c) write the redox half-reactions, and (d) write a balanced net ionic equation. FeI2(aq) + CuI2(aq) −−→ CuI(s) + FeI3(aq)