Thus the transfer of electrons causes the redox reaction to occur. Zn + 2HCl---> ZnCl2 + H2. Which statement correctly describes a redox reaction? H goes from +1 to zero so it is reduced and HCl is the oxidizing agent. problem 1: Zn(s)+Cl2(g)→ZnCl2(s) a...both Zn and Cl are oxidized . HCl is reed. HCl went from +1 to 0, so it is the reduced, and therefore, it is the oxidizing agent. Click hereto get an answer to your question ️ Zn + 2 HCl → ZnCl2 + H2 ↑ The above reaction is an example of: Question: In The Reaction Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) The Oxidation State Of Zn Changes From 0 To +2, And Zn Is Oxidized The Oxidation State Of Zn Changes From 0 To +2, And Zn Is Reduced The Oxidation State Of Zn Changes From 0 To -2, And Zn Is Oxidized The Oxidation State Of Zn Changes From 0 To -2, And Zn Is Reduced electrons. Source(s): https://shrink.im/a0Udy. d....both Zn and Cl are reduced . 0 … n the following reactions, identify what is oxidized, and what is reduced. 4 years ago. Here are some videos to help you understand this concept: Chemistry Tutorial 12.1a: Determining Oxidation Numbers Zn went from 0 to +2, so it is oxidized, and therefore, it is the reducing agent. Explanation: The equation has one reactant's atom(s) given to the other reactant, causing a single replacement. What type of reaction is Zn + 2HCl > ZnCl2 + H2? Zn goes from no charge to +2 so Zn is oxidized and Zn is the reducing agent. Zn 2hcl Zncl2 H2. Personally I prefer to think of it in terms of oxidation and reduction as this more accurately represents the actual species taking part and the transfer of electrons which is the basis of all chemistry. Zn + 2HCl ---> ZnCl2 +H2. Zn + 2HCl -----> ZnCl2 + H2. Half Reaction. When zinc metal is submerged into a quantity of aqueous HCl, the following reaction occurs (Figure 5.4 "Zinc Metal plus Hydrochloric Acid"):Zn(s) + 2HCl(aq) → H 2 (g) + ZnCl 2 (aq). Fe(S) + S(S) ---> FeS(S) Oxidation-Reduction reactions occur because of the competition between particles for. Left: Zn 0 H 1 Cl -1 Right: Zn 2 Cl2 -1 H 0 Zinc is oxed. 34. How do I … Start with an oxidation-reduction equation Zn + 2HCl → ZnCl2 + H2 Separate the reaction into oxidation and reduction half-reactions Zn → Zn^2+ 2H^+ → H2 Confirm that all atoms are balanced. Then, balance the charges with electrons. Which balanced equation represents an oxidation-reduction reaction? An equation showing either the oxidation or the reduction that takes place in a redox reaction - shows e- lost and e- gained. Oxidized: Cl-Reduced: Mn +4 ... O Agent: Cl2 R Agent: NaBr. zinc loses electrons to the electronegative atom Cl with the reaction for oxidation and reduction as follows: Oxidation: Zn→Zn2+ + 2e-Reduction: 2H+ + 2e- →H2. I need to balance the following equation. problem 2: -----... 2PbO(s)→2Pb(s)+O2(g) a)...both O and Pb are reduced . Zn + 2HCl → ZnCl2 + H2. 0 ----- +1 -1 ----- +2 -1 --- 0. Chemistry. Clis -1 on both sides of the equation so it is neither oxidized nor reduced. Chemistry check. Answer link. Related questions. Lv 4. 0 4. leeman. MnO2 + 4HCl---> MnCl2 + 2H2O + Cl2. I just want to make sure I', right: Zn + HCl-> ZnCl2 + H2 Zn + 2HCl-> ZnCl2 + H2 . b...Zn is oxidized, Cl is reduced . In the reaction:Zn+ 2HCL>ZnCl2+h2.What mass ZnCl2 is produced when 10g of zn reacted . science help Equation #2 Zn + HCl --> ZnCl2 + H2 is the correct equation. c...Cl is oxidized, Zn is reduced . 1 Answer Phiri Apr 25, 2018 Single Replacement.