5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water...
Sodium reacts with water according to the reaction: 2Na(s)+2H2O(l)→2NaOH(aq)+H2(g) Identify the oxidizing agent. a) H2O(l) b) NaOH(aq) c) Na(s) d) H2 (g)
HNO3 (aq) + Cu (s) + H2(g) + CuNO3 (aq) •Identify what type of reaction it is: precipitation, redox or acid-base. •Balance the above equation. •Write the balanced net ionic equation. d. Indicate the element that has been oxidized and the one that has been reduced. You should also identify the oxidation number (ox #) of each before and after the process. Identify the reducing agent and the oxidizing agent. Element Oxidized: Ox # Reactant: Ox # Product: Element Reduced:...
Classify each of the following redox reaction as a combination, decomposition, or displacement reaction. Give a blanaced molecular equation for each, as well as total and net ionic equations for parts (b) and (c), and identify the oxidizing and reducing agents. A) S8(s)+F2(g)=SF4 Reaction? Molecular Equation- ? Reducing agent-? Oxidizing agent-? B)Fe(s)+HCl(aq)=FeCl3(aq)+H2(g) Reaction-? Molecular Formula-? Reducing agent-? Oxidizing agent-? Total Ionic Equation-? Total Net Equation-? C) Cu(s)+AgNO3(aq)=Cu(No3)2(aq)+Ag(s) Reaction-? Molecular Formula-? Reducing agent-? Oxidizing agent-? Total Ionic Equation-? Total Net Equation-?
The following is a redox reaction, which takes place in acidic solution: Fe (s) + HC1 (aq) = HFeCl4 (aq) + H2 (g) The oxidation half-reaction is: The reduction half-reaction is: The oxidizing agent is the reducing agent is: The total number of electrons transferred in the balanced redox reaction is Can you please explain how you get everything please! I have the answers i just don't understand how to get there
Write the half-reactions and the net ionic equations for these complete redox reactions 4 2NaCl (aq) + Br: (I) Cl: (g)2NaBr (aq) a) Oxidation half-reaction: Reduction half-reaction: CrCls (aq)+ Au (s) AuCl3(aq) Cr (s) - b) Oxidation half-reaction: Reduction half-reaction: Identify the oxidizing agent and the reducing agent in these complete redox reactions: 5. 5SO2-2Mn2+ 5so +3H2O a) 2MnO, +6H A) MnO B) So2 C) Mn2 D) SO E) H Oxidizing agent: b) 5Fe2 (aq) + MnO4 (ag) +8H'(aq)-5Fe (ag)+...
Name: Lab Section: 1 2 3 4 5 6 7 8 Report: Redox Reactions 1. Consider the following balanced redox reaction: 2 Li (8) + CuCl(aq) + Cu (8) + 2 LCI (a) a. Write the oxidation number for each element in the spaces below each species. b. Which element is... Oxidized Reduced C. Which reagent is the... Oxidizing agent? Reducing agenti d. Each Li atom (gains / loses) electron(s) and each Custom (gains / loses) e. In the overall...
Problem Page Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. redox reaction? yes no 2H, $...
1. For the oxidation-reduction reaction Zn(s) + 2HNO3 (aq) → H2(g) + Zn(NO3)2 (aq) Hint: HNO3 a) provide equation for the oxidation half-reaction: b) provide equation for the reduction half-reaction: In the given equation above or in your answers to a) and b): c) label the substance which is oxidizing agent, d) label the substance which is reducing agent.
Consider the following half-reactions: Half-reaction E° (V) 12(s) + 2e - →21"(aq) 0.535V 2H+ (aq) + 2e - → H2(g) 0.000V Cr3+(aq) + 3e —— Cr(s) -0.740V The strongest oxidizing agent is: enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will 12(s) reduce Cr3+(aq) to Cr(s)? — Which species can be reduced by H2(g)? If none, leave box blank. Use the References to access important values if needed for this question....
Consider the following redox reaction MnO4- + SO32- —→ SO42- + MnO2 a) Write a balanced oxidation half reaction b) Write a balanced reduction half reaction c) Which species is the oxidizing and reducing agents d) Write the overall BALANCED ionic equation UNDER BASIC CONDITIONS