Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redoxreaction, write down the formula of the reducing agent and the formula of the oxidizing agent.2C1₂(g) + Sn(s) →SnC14 (s)CuSO (aq) + Zn (s) → ZnSO₂ (aq) + Cu (s)42N₂(g) + 50₂(g) 2N₂O₂(g)redox reaction?yesreducingagent:oxidizingagent:redox reaction?yesreducingagent:oxidizing Пagent:redox reaction?yesreducing 0agent:oxidizing 0agent:nononoX00Ś

Redox reaction : Chemical reactions involving both oxidation and reduction processes. During a redox…

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. 2C1₂(g) + Sn (s) CuSO4 (aq) + Zn (s) → ZnSO4 (aq) + Cu (s) 2N₂(g) + 50₂(g) SnCl (s) - 2N₂05 (8) redox reaction? O yes reducing agent: oxidizing agent: redox reaction? O yes reducing agent: oxidizing agent: O yes Ono redox reaction? reducing agent: oxidizing agent: Ono no X

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. 2C1₂(g) + Sn (s) CuSO4 (aq) + Zn (s) → ZnSO4 (aq) + Cu (s) 2N₂(g) + 50₂(g) SnCl (s) - 2N₂05 (8) redox reaction? O yes reducing agent: oxidizing agent: redox reaction? O yes reducing agent: oxidizing agent: O yes Ono redox reaction? reducing agent: oxidizing agent: Ono no X

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The first reaction is of a strong oxidizer (HNO3) with a metal (Cu) to produce copper nitrate, nitrogen dioxide, and water. Indicate the oxidation state of each element (atom) in the reactants and products. Describe which species was oxidized, and which species was reduced in this reaction (where did the electrons come from and where did they go?). (Reaction 1) Cu(s) + HNO3(aq) → Cu(NO3)2(aq) + H2O(l) + NO2(g)
A 4.50 g sample of limestone (impure CaCO3) was dissolved in 0.1M HCl solution according to the following equation. CaCO3(s) + 2HCl(aq) → CaCl2 (aq) + CO2 (g) + H2O (l) Excess of (NH4)2C2O4(aq), was added to the resulting solution to precipitate the calcium ions as calcium oxalate, CaC2O4(s). Ca2+(aq) + C2O42-(aq) → CaC2O4 (s) The precipitate was filtered, dried and weighed at 2.15 g. (Show your work) a) Determine the percentage by mass of calcium carbonate (CaCO3) in the limestone sample. (MM of CaCO3 is 100.09 g/mol) b) Why we need to dry the precipitate until we get a constant mass? c) Is the precipitate of calcium oxalate (CaC2O4) stable and in the final form or not? Explain.
When potassium cyanide (KCN) reacts with hydrochloric acid, a poisonous gas of hydrogen cyanide is given off. The equation describing this process is: KCN(aq) + HCL(aq) ==> KCl(aq) + HCN(g) If 0.140 g pf KCN is completely reacted with hydrochloric acid, calculate the amount of HCN that is formed.
Redox Reactions
The following reaction occurs when two aqueous solutions are mixed: Cr(NO3)3(aq) + 3NaOH(aq) → Cr(OH)3(s) + 2NaNO3(aq) Identify the spectator ion OR ions in the solution. SELECT ALL SPECTATOR IONS!
Write the net ionic equation for the reaction of copper(II) sulfate with sodium sulfide. A) 2 Cu⁺ (aq) + SO₄²⁻ (aq) → Cu₂SO₄ (s) B) 2 Na⁺ (aq) + SO₄²⁻ (aq) → Na₂SO₄ (s) C) Cu²⁺ (aq) + S²⁻ (aq) → CuS (s) D) 2 Cu⁺ (aq) + S²⁻ (aq) → Cu₂S (s)
When this equation: Fe(s) + AgNO3(aq) → Ag(s) + Fe(NO3)2(aq) is balanced, the net ionic equation is: a. 2Fe(s) + 2Ag*(aq) → 2Ag(s) + 2FE2"(aq) b. 2Fe(s) + Ag*(aq) → Ag(s) + 2FE2"(aq) c. Fe(s) +2 NO; (aq) - → Ae) 2NO3 (i1;) 37. CS Scand F(s, 2Ag"(aq) → 2Ag(s) + Fe“(aq) e. None of the above
Balance the "molecular" equation for the above reaction: Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1)
Consider the reaction shown below between hydroxide ions (OH), hypochlorite ions (CIO), and chromium hydroxide ions (Cr(OH)4): 2 OH (aq) + 3 CIO (aq) + 2 Cr(OH)4 (aq) → 3 CI (aq) + 5 H₂O (1) + 2 CrO4² (aq) Which atom was oxidized during this reaction? [Select] Which atom was reduced during this reaction? [Select] Which substance was the oxidizing agent in this reaction? [Select] Which substance was the reducing agent in this reaction? [Select]
Consider the following balanced redox reaction:16H⁺(aq) +2MnO₄⁻(aq) +10Cl⁻(aq) →2Mn²⁺(aq) +5Cl₂(g)+ 8H₂O(l)(a) Which species is being oxidized?(b) Which species is being reduced?(c) Which species is the oxidizing agent?(d) Which species is the reducing agent?(e) From which species to which does electron transfer occur?(f ) Write the balanced molecular equation, with Kand SO₄²⁻ as the spectator ions
Cr(OH)3 (s) + Cl2 (g) → Na2CrO4 (aq) + NaCl (aq) balance in basic solution
W Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. O 2 H* (aq) + CO3²-(aq) → H₂CO3(s) 2 Na* (aq) + CO3²- (aq) + 2 H*(aq) + 2 CÃ¯(aq) → H₂CO3(s) + 2 NaCl(aq) O 2 H* (aq) + CO3²-(aq) → H₂O(1) + CO₂(g) 2 Na* (aq) + CO3²- (aq) + 2 H* (aq) + 2 Cl(aq) → H₂CO3(s) + 2 Na*(aq) + 2 Cl(aq) No reaction occurs.