In Part A of the experimental procedure, copper metal is added to concentrated nitric acid. The reaction between copper metal and concentrated nitric acid is an oxidation-reduction reaction that is somewhat complicated. 4 HNO3(aq) + Cu(s) → Cu(NO3)2 (aq) + 2 H₂O (1) + 2 NO₂ (g) Consider the balanced chemical reaction given above. Assign the oxidation numbers to each atom in the equation. Cu: H: O: N: 4 HNO3(aq) +1 -2 +5 ✓ Which element undergoes OXIDATION? 0 I. 2. OXIDIZING AND REDUCING AGENTS 1. 3. ELECTRON TRANSFER Which element undergoes REDUCTION? + Cu(s) Cu(NO3)2 (aq) +2 -2 +5 2 2 + 2 H₂O (1) +1 -2 How many moles of electrons are transferred between the elements being oxidized and reduced? +2 NO₂ (g) -2 +4 ✓

In Part A of the experimental procedure, copper metal is added to concentrated nitric acid. The reaction between copper metal and concentrated nitric acid is an oxidation-reduction reaction that is somewhat complicated. 4 HNO3(aq) + Cu(s) → Cu(NO3)2 (aq) + 2 H₂O (1) + 2 NO₂ (g) Consider the balanced chemical reaction given above. Assign the oxidation numbers to each atom in the equation. Cu: H: O: N: 4 HNO3(aq) +1 -2 +5 ✓ Which element undergoes OXIDATION? 0 I. 2. OXIDIZING AND REDUCING AGENTS 1. 3. ELECTRON TRANSFER Which element undergoes REDUCTION? + Cu(s) Cu(NO3)2 (aq) +2 -2 +5 2 2 + 2 H₂O (1) +1 -2 How many moles of electrons are transferred between the elements being oxidized and reduced? +2 NO₂ (g) -2 +4 ✓

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

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. 3Cr(NO3), (aq) + 2Al(s) 3Cr(s) + 2A1(NO3)₂(aq) 2 HCl(aq) + NH₂ (aq) → NH₂Cl(aq) 3 2Na (s) + Cl₂ (g) 2 Na Cl (s) redox reaction? yes reducing agent: oxidizing 0 agent: redox reaction? yes reducing agent: 0 oxidizing 0 agent: redox reaction? yes reducing 0 agent: oxidizing 0 agent: no no no X On Ś
Identify the elements that undergo changes in oxidation number in the following reaction: 2H2SO4(aq)+2NaBr(s)→Br2(l)+SO2(g)+Na2SO4(aq)+2H2O(l) Express your answers as chemical symbols separated by a comma. S,Br, O = marked wrong. Says insufficient items
Give the complete ionic and net ionic equation for the reaction below. Circle the spectator ions. Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq)
3. For each of the following balanced equations, write the oxidation number below the symbol of each atom that changes oxidation state in the course of the reaction. a) 2 PF21 (1) + 2 Hg (I) → P2F4 (g) + Hg2l2 (s) b) 2 KCIO3 (s) → 2 KCI (s) + 3 O2 (g) c) 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H2O (g) d) 2 As (s) + 6 NaOH (I) → 2Na3AsO3 (s) + 3H2 (g)
Choose which of the given equations is a oxidation-reduction (redox) disproportionation reaction. 5 NaBr(aq) + NaBrO3(aq) + 3 H₂SO4 (aq) → 3 Na₂SO4 (aq) + 3 Br₂ (1) + 3 H₂O(1) 2 O CH₂(g) + 2O₂(g) CO₂(g) + 2 H₂O(g) ○ 2H₂O₂(1) → ○ 2 H₂PO4 (aq) HPO2 (aq) + H₂PO4 (aq) 2H₂O(1) + O₂(g)
A displacement reaction is an oxidation-reduction reaction in which a free element reacts with a compound, displacing an element from it. This is an example of such reaction: Sn(s) + 2HCI(ag) → SnCla (aq) + H2 (9) b Give the formula of the oxidizing agent. Formula:
Write the net ionic equation for the following molecular equation. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)
3Cr(NO₂), (aq) +2A1(s)-3Cr(s) + 2AI (NO₂), (ag) 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. 2AgNO, (ag) + CaCl, (aq) - 2 AgCI(1) + Cu(NO₂), (4) 2N, (e) + 50, (e)- 2N, 0, (e) redox reaction? O yes reducing O agent: oxidizing 0 agents redox reaction? O yes reducing 0 agent: oxidizing 0 agent redox reaction? yes reducing agent: oxidizing agent: no no O no 015 X Jalm
Assigning oxidation numbers Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom oxidation state of species highlighted atom VO(s) Cu (aq) %3D
A student combined CuCl2 (aq) and Na (s). The student observed a color change, thus a reaction occurred. Write the balanced molecular equation for this reaction showing coefficients and phase labels. Write the complete ionic equation for this reaction. Write the net ionic equation for this reaction. Assign oxidation numbers to the reactants and products in the net ionic equation. Which reactant, CuCl2 (aq) or Na (s), got oxidized? Which reactant, CuCl2 (aq) or Na (s), got reduced? Which reactant, CuCl2 (aq) or Na (s), is the oxidizing agent? Which reactant, CuCl2 (aq) or Na (s), is the reducing agent?
Using the reaction 2Al(s) + 3CuCl2·2H2O(aq) -> 3Cu(s) + 2AlCl3(aq) + 6H2O(l), complete the oxidation numbers for each element in the table and determine the
Balance the molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and states of the products in each of the cases. CaCl2 (aq) + Pb(OH)2 (aq) → H2SO4 (aq) + Ba(OH)2 (aq) - AGNO3 (aq) + KCI (aq) – HCIO4 (aq) + Ca(OH)2 (aq) -