6.) Consider the following half-reaction containing acid HX below.3 N2 (g) + 2 H (aq) +2 e 2 HX (aq)E°= -3.09 VA. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HXbehave like an active metal?B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, O,.O, (g) + 2 H (aq) +2 e > 02 (g) + H:O () E'red =2.076 VCould HX be applied to mitigate ozone, O, (g), depletion in the atmosphere? Write the balanced equation for the reactionused and explain why or why not using your calculated E". value.C. How does your reaction equation in B support your answer to A?D. Calculate both AG° support your answer to B.

Solution: A) Yes, we can see the standard reduction potential is - 3.09 V. Since we know standard…

6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H (aq) +2 e → 2 HX (aq) Ered =-3.09 V A. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HX behave like an active metal? B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, Og. O: (g) + 2 H (aq) +2 e 02 (g) + H2O (1) E°red =2.076 V Could HX be applied to mitigate ozone, O, (g), depletion in the atmosphere? Write the balanced equation for the reaction used and explain why or why not using your calculated E°cell value. C. How does your reaction equation in B support your answer to A? D. Calculate both AGo support your answer to B.

6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H (aq) +2 e → 2 HX (aq) Ered =-3.09 V A. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HX behave like an active metal? B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, Og. O: (g) + 2 H (aq) +2 e 02 (g) + H2O (1) E°red =2.076 V Could HX be applied to mitigate ozone, O, (g), depletion in the atmosphere? Write the balanced equation for the reaction used and explain why or why not using your calculated E°cell value. C. How does your reaction equation in B support your answer to A? D. Calculate both AGo support your answer to B.

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

Please don't provide handwritten solution...
2. Tell whether each of these statements are true and false. If false, rewite it to make it a correct statement. Oxidation always occurs at the anode of an electrochemical cell. The anode of a voltaic cell is the ite of reduction and is negative. Standard conditions for electrochemical cells are a concentration of 1.0 M for disolved species and a pressure of 1 bar for gases. The potential of a voltaic cell does not change with temperature. All product-favored oxidation-reduction reactions have a standard cell voltage E°cell, with a negative sign.
3q112 please answer with solutions thanks
7
Element A has a standard reduction potential of +0.74V, whereas Element B has a standard reduction potential of -1.15V. Which of the following statements is correct with respect to building a Galvanic cell with these two elements? A. A will be the cathode, B will be the anode, and the cell potential will be positive. B. A will be the cathode, B will be the anode, and the cell potential will be negative. C. A will be the anode, B will be the cathode, and the cell potential will be positive. D. A will be the anode, B will be the cathode, and the cell potential will be negative. E. The anode, cathode, and cell potential must all be experimentally determined.
Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?
Help with the following question
1. Consider the following standard reduction potentials in acid solution: E°(V) -1.66 +0.07 +0.14 Fe³+ + e +0.77 The strongest reducing agent among those shown above is Hint: If answer is with charge, type this way: X2+ Al³+ + 3e → Al(s) AgBr(s) + e → Ag(s) + Brā Sn4+ + 2e → + 2e → Sn²+ Fe²+
A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.
Enter electrons as e". Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and Cl,(g), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.
Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur when Sn metal is put into a 1M aqueous Co2* solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank. >
Oo.98. Subject :- Chemistry