First, balance the half-reactions with respect to atoms other than hydrogen and oxygen (if needed) by inserting coefficients. Then, balance oxygen and Balance the equation in basic conditions. Phases are optional. hydrogen as needed by adding H, 0 and OH-. Then, balance the charge by equation: so + Co(OH), SO → +CO + H,0 adding electrons to the more positive side. Incorrect so?- so > Co(OH), » Co If the half-reaction involves a metal hydroxide, just add OH- ions. Otherwise, add twice as many OH- ions as needed to balance O, then half that number of H,0 molecules to the opposite side. Once you have the two balanced half-reactions, multiply one or both of them by a small integer so that the electrons will cancel out when you sum the half-reactions. ALTERNATE METHOD: First, balance the half-reactions with respect to atoms other than hydrogen

First, balance the half-reactions with respect to atoms other than hydrogen and oxygen (if needed) by inserting coefficients. Then, balance oxygen and Balance the equation in basic conditions. Phases are optional. hydrogen as needed by adding H, 0 and OH-. Then, balance the charge by equation: so + Co(OH), SO → +CO + H,0 adding electrons to the more positive side. Incorrect so?- so > Co(OH), » Co If the half-reaction involves a metal hydroxide, just add OH- ions. Otherwise, add twice as many OH- ions as needed to balance O, then half that number of H,0 molecules to the opposite side. Once you have the two balanced half-reactions, multiply one or both of them by a small integer so that the electrons will cancel out when you sum the half-reactions. ALTERNATE METHOD: First, balance the half-reactions with respect to atoms other than hydrogen

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

Write a half-reaction for the oxidation of the manganese in MNCO3(s) to MnO2(s) in neutral groundwater where the carbonate-containing species in the product is HCO3 (aq). Add H2O and H* to balance the H and O atoms in the equation. Do not add electrons; you may leave the half-reaction unbalanced with respect to charge. X X. Не (aq),
please help me to answer this question and show all work so that i may understand, thank you!
For each of the following balanced oxidation-reduction reactions,(ii) state the total number of electrons transferred in each reaction. (Can you please show me how step by step, I keep getting stuck trying to balance the half reactions) (a) I2O5 +5 CO ---> I2 + 5 CO2 (b) 2Hg2+ + N2H4 ----> 2 Hg + N2 + 4 H+ (c) 3 H2S + 2 H+ + 2 NO3- -------> 3 S + 2 NO + 4 H2O Group of answer choices
I need help with the final question which is in bold. The previous questions and answers are needed to answer the final question In an electrolysis experiment similar to the one employed this experiment; a student observed that his unknown metal anode lost 0.238 grams while a total volume of 94.50 mL of hydrogen was being produced. The temperature of the solution was 25oC and the barometric pressure was 739 mm Hg. The difference between the water levels in the beaker and buret was negligible. The vapor pressure of water at 25oC is 23.8 mm Hg. Based on the information provided and the lab handout, what pressure of hydrogen is collected, in atmospheres? 9.41x10^-1 atm Using the data collected (in the previous problem), calculate the moles of hydrogen collected. 3.63x10^-3 mol Upon electrolysis, the metal is oxidized to a 2+ valence state. Based on this information, how many moles of metal are present? 3.63x10^-3 mol Use the mass of metal lost and moles from the previous problem to…
I need help with all parts. Thanks
For the following reaction, write the half-reactions, stating which is the reduction half-reaction andwhich is the oxidation half-reaction. 2H+ + H2O2 (el) + 2I- (aq) → I2 (s) + 2H2O (el)
Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP"(1.00M) | Pb³"(1.00M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al"] to have changed by 0.60 mol/L. (Assume T = 25°C.) (b) Many elements have been synthesized by bombarding relatively heavy atoms with high-energy particles in particle accelerators. Complete the fol- lowing nuclear equations, which have been used to synthesize elements. U + C-→ Cf + Cf + 'B Lr + + He Bk + in + 6 n 10 Db + 4 in 103
When balancing equations for redox reactions in acidic solutions, which of the steps comes before you balance each half-reaction for O by adding H20? O Balance each half-reaction for charge by adding electrons Balance each half-reaction for H by adding H* Balance each half-reaction for all elements except H and O Write skeletal equations for the oxidation and reduction half-reactions
In an car battery recharging occurs when the car is running by supplying a current to the battery. The reaction that occurs at the cathode in this electrolytic process is Pb2+ + 2e- --> Pb (s) If the car supplies a current of 1.50A to the battery, how long will it take in minutes to have 25.0 g of Pb(s) collected at the cathode? Hint: Start with 25.0 g Pb (1A = 1C/sec) (F= 96500 C/mole e-) (Pb =207.2g/mol) Answer has 3 sig figs
Complete and balance the following half-reaction in basic solution H,0(1) + SO,²(aq) + 2 e SO (aq) + 2 H,O(1) -> 3 2. 2+ 3+ O4+ 4- n3- 56 78 6. 0 1 3 口3 Os 06 07 8. O2 4 (s) (1) (g) (aq) H,O OH- H+ e H. SI 1L 2. 4. 2.
Consider the following half-reactions: (1) The weakest oxidizing agent is: (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will Mg(s) reduce F₂(g) to F'(aq)? | + Half-reaction F₂(g) + 2e 2H+(aq) + 2e™ Mg2+ (aq) + 2e™ (6) Which species can be reduced by H₂(g)?| If none, leave box blank. E° (V) 2.870V H₂(g) 0.000V Mg(s) -2.370V 2F (aq) enter formula
Consider the following half-reactions: (1) The strongest oxidizing agent is: (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Fe²+ (aq) oxidize F'(aq) to F₂(g)? ◆ (6) Which species can be reduced by Ni(s)?| If none, leave box blank. Half-reaction F₂(g) + 2e Ni2+(aq) + 2e Fe²+ (aq) + 2e™ E° (V) 2F (aq) 2.870V Ni(s) -0.250V Fe(s) -0.440V enter formula