Balance the following ionic equation using the half reaction method. Be sure to show the steps in obtaining the balanced oxidation and reduction half reactions. Note: More than one atom may be either oxidized or reduced. If so, write a separate reaction for each atom which changes its oxidation state. Cl + F + S2O8²Cl2 + F2 + SO4²- -

Write the oxidation and reduction half reactions for the following redox reaction. Make sure to label which is the oxidation and which is the reduction. (The number of electrons in both half reactions should be equal. You may balance the equation first if it helps you.) Al s)+HCI aq) → AIC 1, aq +H,(g) Write the ionic equation and net ionic equation for the following reaction. (Make sure to balance the equation.) Na,CO, aq+CaCl, aq) - NaCl aq+CaC O,(s) Determine the concentration in mol/L (M) of a solution of 19 25 g of LICLin acO O

Type in each of the following equations as it is shown in the text box using ChemType. Subscripts need to be subscripts and superscripts need to be superscripts. Chemical arrows must be used. You should have written fourteen equations when you are done. BALANCING REDOX REACTIONS Example #6 Balance the following redox reaction which occurs in a basic solution: SO3²- + MnO4 → SO₂²- + MnO₂ Which half-reaction is reduction? Which is oxidation? Separate into two skeleton half equations SO3²- → SO₂2- F3 MnO → MnO₂ MnO → MnO₂ + 2H₂O 4 4H+ + MnO₂ → MnO₂ + 2H₂O MnO4 → MnO₂ 4H+ + MnO + 4OH → MnO₂ + 2H₂O + 40H- 4H₂O + MnO₂ → MnO₂ + 2H₂O + 40H- MnO₂ + 2H₂O + 40H- 4 20 F4 % 5 2OH- + SO3²- + H₂O → SO2 + 2H+ + 2OH- 2OH- + SO3²- + H₂O → SO2 + 2H₂O 20H-+SO3²- + H₂O → SO2 + 2H₂O + 2e- 4H₂O + MnO4 + 3e 21 O Search SO3² + H₂O → SO₂²- 2- SO3 + H₂O → SO2 + 2H+ F5 A 6 F6 & 7 ▶ || F7 ★ 8 WHICLE F8 9 F9 0

3. Write the half-reactions (labelled as oxidation or reduction) for the following equation: Znjs) + 2 AGNO3(aq) → Zn (NO3)2(ag) +2 Ag(s)

KClO2⟶KCl+O2KClO2⟶KCl+O2   assign oxidation numbers to each element on each side of the equation.

Balance the following using the half-reaction method. Identify oxidation, reduction, reducing agent, oxidizing agent. i. Be(NO3)2 (aq) + Ce(s)--> Ce(NO3)3(aq) + Be(s) ii. A container contains H2SO3, H2SO4, Pb2+, Pb4+ and NO3- in distilled water. Create a balanced chemical reaction (Net Ionic Equation, including states of matter) for the spontaneous reaction in the container

You are tasked with creating a pourboix diagram of sulfur speciation. The relevent species are SO42-, HSO42-, S, H2S, and HS-. The total copper is 10^-6 mol. Set and balence the redox reactions needed for this question and explain how you landed on those reactions.

Balance the following oxidation-reduction reactions. In Basic solution _Ni²+ (aq) + 2- _Cr(OH)3(s) =>____Ni(s) + ______CrO4²- Type out the balanced equation to the best you can or write out where the coefficients and added water would be.

So we are doing a lab to show how, in principle, pure metal is pulled out of ore from the ground. This is where you take Cu(s) and react it with HNO3(aq) and then a bunch more reactions to get Cu(s) back.  All I am looking for is to make sure that I am doing the 'half-reaction' method correctly to get a balanced net ionic equation. The information given is this: Oxidation: Cu(s) -> Cu2+(aq) + 2e- Reduction: NO3-(aq) + e- -> NO2 (g) It also notes that this is in an acidic environment so there are excess H+ in solution. so to balance the mass in the reduction side of things I added H2O (since you are starting with HNO3 there will be 2H+ for the water molecule anyway, but they can come from anywhere) so now it looks like: Oxidation: Cu(s) -> Cu2+(aq) + 2e- Reduction: NO3-(aq) + e- -> NO2 (g)+ H2O(l) now the reduction needs to be multiplied by 2 so the charges cancel out: Oxidation: Cu(s) -> Cu2+(aq) + 2e- Reduction: 2NO3-(aq) + 2e- -> 2NO2 (g)+ 2H2O(l) Now the 2…

1- Balance the following redox reactions using the oxidation number method a. NaClO + H2S = NaCl + H2SO4 b. Sn + HNO3 + H2O = H2SnO3 + NO   2- Balance the following redox reactions using the half-reaction method. a. Mg + Al+3 = Mg+2 + Al b. H2O2 + Cr2O72- = O2 + Cr+3 (in acidic solution)   2.Rank the following entities in order of increasing strength as oxidizing agents. (1=weakest oxidizing agent and 6= strongest oxidizing agent) Cd+2(aq)                   IO3-1(aq)                 K+1(aq)                       H2O(l)                    AuCl4-1(aq)                     I2(s)   3. Indicate which of the following pairs of substances, when combined, will result in a spontaneous chemical reaction. Write spontaneous or non-spontaneous. a.    K+1(aq) and Na(s)                   b.   Cr+2(aq) and K(s)                   c.    Pb+2(aq) and Fe(s)           d.   Ag(s) and Sn+2(aq)