Q. 1Write balanced net ionic equations for the following reactions. Supply H* and/or H,0 as needed toobtain balance.MnO4 +H,SO, Mn2t +SO,2-Ti + Fe(CN), TiO + Fe(CN),+Q. 2Identify the oxidizing agent and the reducing agent on the leftside of each equation in Q. 1; write a balanced equation for eachhalf-reaction.

Since you have asked multiple questions, we are solving first question for you. For remaining…

Write balanced net ionic equations for the following reactions. Supply H and/or H,O as needed to obtain balance. MnO, +H,SO, Mnt +SO,2- Tyt + Fe(CN), TiO +Fe(CN), Q. 2 Identify the oxidizing agent and the reducing agent on the left side of each equation in Q. 1; write a balanced equation for each half-reaction.

Write balanced net ionic equations for the following reactions. Supply H and/or H,O as needed to obtain balance. MnO, +H,SO, Mnt +SO,2- Tyt + Fe(CN), TiO +Fe(CN), Q. 2 Identify the oxidizing agent and the reducing agent on the left side of each equation in Q. 1; write a balanced equation for each half-reaction.

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

Use the standard reduction potentials given below to predict if a reaction will occur when Fe metal is put into a 1 M aqueous Cd²+ solution. Cd²+ red (aq) + 2e¯ → Cd(s) Ee Fe²+ (aq) + 2e → Fe(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) -0.403 V -0.440 V + +
Balance the following in basic solution. Lowest possible coefficients. Omit phases. Show oxidation reaction, reduction reaction and net reaction. Zr(OH)2(s) + O2(g) --> ZrO2(s) N2O4(aq) + H2(g) --> NO(g)
Consider the following redox reaction: Cl207 (aq) + H2O2 (aq) ClO2 (aq) + 02 (g) -> a. Allocate oxidation states to all the elements in the reaction b. Identify the oxidizing and reducing agents c. Balance the redox reaction in an acidic medium using the half-reaction method
Use standard reduction potentials to calculate the equilibrium constant for the reaction: Fe (aq) + H2(g) Fe(s) + 2H (aq) Hint: Carry at least 5 significant figures during intermedliate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG" for this reaction would be than zero.
Use the standard reduction potentials given below to predict if a reaction will occur when Al metal is put into a 1 M Fe²+ solution. aqueous Fe2+ (aq) + 2e → Fe(s) E red Al³+ (aq) + 3e →→ Al(s) E + red = If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. ― -0.440 V -1.660 V (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- → La (s) E° = -2.37 V Na+ (aq) + e- → Na (s) E° = -2.71 V 1.8 x 10-6 5.7 x 10-18 5.6 x 105 1.7 x 1017
29b
Balance the following redox equation to its lowest integer ratio. (Under Acidic Conditions) Te(s) + Ru(NO3)3(aq) + NO2(g) ↔ Ru2Te3(s) + HNO3(aq) Note that H2O and H+ are not shown in the equation above. If it is required to balance the equation, then add these.Fill in the coefficient for each chemical after you finish balancing the equation. If the chemical is not needed in the equation then mark a zero next to it Te(s) HNO3(aq) H2O(l) Ru2Te3(s) NO2(g) Ru(NO3)3(aq) H+ (aq)
Use the standard reduction potentials located in the Tables' linked above to calculate the standard free energy change in kj for the reaction: Fe²+ (aq) + Hg(1)→ Fe(s) + Hg²+ (aq) Answer: 237.16 K for this reaction would be greater than one.
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?
Write a balanced half-reaction for the reduction of CrO 4 2–(aq) to Cr(OH) 3(s) in a basic solution.
Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy delta G^0 for the following redox reaction. I2(s) + 6H2O(l) + 5 Cl2(g) -> 2IO3-(aq) + 12H+(aq) + 10Cl-(aq)Be sure your answer has the correct number of significant digits.