(Q81) The oxidation number for nitrogen in a certain reaction goes from +5 to -2 and the oxidation number for sulfur goes from -1 to +4. Which of the following statements is true? Electrons moved from nitrogen to sulfur Nitrogen has been reduced and sulfur has been oxidized O This reaction could not take place because oxidation numbers cannot be negative Both nitrogen and sulfur have been reduced Nitrogen has been oxidized and sulfur has been reduced

(Q81) The oxidation number for nitrogen in a certain reaction goes from +5 to -2 and the oxidation number for sulfur goes from -1 to +4. Which of the following statements is true? Electrons moved from nitrogen to sulfur Nitrogen has been reduced and sulfur has been oxidized O This reaction could not take place because oxidation numbers cannot be negative Both nitrogen and sulfur have been reduced Nitrogen has been oxidized and sulfur has been reduced

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

Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as a chemical formulas. Omit states-of-matter. Zn(s) + 2Ag* (aq) → 2 Ag(s) + Zn2+ * (aq) а. Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced No v b. HBr(g) + NH3 (g) → NH,Br(8) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes v С. GeCl4 (1) + 2H2O(1) → 4HC1(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si Br4 (1) + 2Ba(s) → 2BAB12 (s) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Ga(OH), (ag) - → GaO2 (ag) + 2H2O(1) е. Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Previous Next
For the reaction: Br2 + ClO– → Br– + ClO3– Which species is oxidized? ClO– Br2 ClO3– Which species is the oxidizing agent? ClO– Br2 Br–
For each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. Write the chemical formulae of any reactants that will be reduced in the third column. reactants reactants reaction oxidized reduced 2Cu(s) + I, (s) → 2CuI (s) 0, (8) + Cr(s) → Cro, (s) 8Ca (s) + S, (s) → 8CAS (s)
80°F Sunny The oxidation number of an element can vary. O True Search F8 6725 F9 O False - « Οι F10
1) What are the coefficients of the balance equation? 2) What is the total number of electrons lost/gained? 3) What is the substance that undergo oxidation reaction? reduction reaction? 4) Which of the reactants is the oxidizing agent? reducing agent? 5) Which substance was oxidized? reduced? 6) Which compound is the product of oxidation? product of reduction?
1) What are the coefficients of the balance equation? 2) What is the total number of electrons lost/gained? 3) What is the substance that undergo oxidation reaction? reduction reaction? 4) Which of the reactants is the oxidizing agent? reducing agent? 5) Which substance was oxidized? reduced? 6) Which compound is the product of oxidation? product of reduction?
Recognising reduction and oxidation.
Which of the following is an oxidation reduction (redox) reaction? 1. MgCl2 (aq) + Pb(NO3)2 (aq) = Mg(NO3)2 (aq) + PbCl2(s) 2. 2 Zn (s) + FeCl2 (aq) = Fe (s) + 2 ZnCl2 (aq) 3. 2 H2SO4 (aq) + NaOH (s) = 2H2O (l) + Na2SO4 (aq) 4. Na3PO4 (aq) + FeCl3 (aq) = 3NaCl (aq) + FePO4 (s)
How to tell what element is being oxidized and reduced in a redox reaction with no visible charge in the equation? 2Au(s) + 6HCl(aq) = 2AuCl3(aq) + 3H2(g) 4Fe(s) + 3O2(g) = 2Fe2O3(s)
Which substance is oxidized in each reaction? a) 2Zn(s) + O2(g) = 2ZnO(g) b) CH4(g) + 2 O2(g) = CO2(g) + H2O(g) c) Sr(s) + F2(g) = SrF2(s)
Consider the following redox reaction: 3Ag+ (aq) + Al(s) → 3Ag (s) + A1³+ (aq) If this reaction starts with 2.50 g of Al and the enough amount of Ag+, how much of electric charge could be generated? 4.28 x 104 C 8.94 × 10³ C 2.68 × 104 C 6.25 × 10³ C O 1.67 x 104 C
Assign oxidation states to all of the species in the following redox reaction. For the reactants, also identify electron loss or gain, the species oxidized, the species reduced, the oxidizing agent and the reducing agent. Oxidation state Electron gain/loss Oxidized or reduced Reducing or oxidizing agent Mg(s) ♥ ↑ ↑ ♥ + Hg²+ (aq) ♥ ↑ ↑ ♥ Mg2+ (aq) + Hg(1) ◊ Total number of electrons transferred from the reducing agent to the oxidizing agent for the equation given is: