Rälah Sureniz: (Us 28d 12sh ) Ayn anda birden çok oturum açan kullanıcının sinavi geçersiz sayılacaktıri. SORU-11 A BO DIraK I. Corrosion is the event that metals lose their properties as a result of chemical and electrochemical reactions with their environment. II. Oxide and sulfur compounds of metals are the most stable. III. The higher the desire of a metal to turn into an ion, the easier it is for the metal to corrode. IV. Metals with more positive standard reduction potential are considered more active. V. Corrosion can be thought of as a galvanic battery that generates current by itself. Which of the above is/are wrong? Yalnız II A-) Il ve IV B-) I1, V ve IV C-) Yalnız IV D-) L,I ve V E-) O O OO

Rälah Sureniz: (Us 28d 12sh ) Ayn anda birden çok oturum açan kullanıcının sinavi geçersiz sayılacaktıri. SORU-11 A BO DIraK I. Corrosion is the event that metals lose their properties as a result of chemical and electrochemical reactions with their environment. II. Oxide and sulfur compounds of metals are the most stable. III. The higher the desire of a metal to turn into an ion, the easier it is for the metal to corrode. IV. Metals with more positive standard reduction potential are considered more active. V. Corrosion can be thought of as a galvanic battery that generates current by itself. Which of the above is/are wrong? Yalnız II A-) Il ve IV B-) I1, V ve IV C-) Yalnız IV D-) L,I ve V E-) O O OO

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

9. Write a Nernst expression, at 25 °C, for the following half-reactions: (a) Zn* (aq) + 2 e- 5 Zn (s) (b) Fe* (aq) + e- s Fe2* (aq) (c) 2 H* (aq) + 2 e- H2 (g) (d) Cr2O2- (aq) + 6 e + 14 H* (aq) S 2 Cr* (aq) + 7 H2O (I)
Q1
What volume, in liters, of hydrogen gas measured at STP can be produced from 50.0 mL of 6.0 M hydrobromic acid and an excess of zinc metal, according to the following reaction?
Given the following data: FEE Conc. (M) Volume (mL) Tinitial (°C) Tfinal (°C) Solution NaOH 0.750 50.00 19.84 23.18 HCI 0.500 50.00 19.84 Calculate AH° for the reaction: HCl(aq) + NaOH(aq) H2O(1) + NaCl(aq) You may assume all solutions to have the same density and specific heat as water (1.00 g/mL and 4.184 J/g°C) kJ/mol
For the following redox reaction calculate the Ecell and K at 298 K. 2Na+(aq) + Ca(s)→2Na(s) + Ca2+(aq) Half Reaction E(V) Na+(aq) + e- → Na(s) -2.71 Ca2+(aq) + 2e- → Ca(s) -2.87
R = 8.314 mol·K F = 96,485 mot AG = AG° + RT · In(Q) ΔΕΔΕ-).In(O) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (1) 1.229 2 z" (aq) Z2 (s) + 2 e 3+ (aq) + 3 е 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e H2 (g) + 2 OH (aq) - 0.828 G (s) - 1.245 > M2+ (aq) + 2 e - 1.893 → M (s) A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate AG° in kJ/mol for this galvanic cell. Report your answer with 4 significant figures. You do not need to report units with your answer. If your value is negative, make sure to include a "-" symbol.
Calculate AG for the reaction 2 H2S(g) + SO2(g) 53 Sthombic(s) + 2 H2O(g) For the following conditions at 25°C: PH,s=0.0001 atm Pso; =0.0290 atm PH,0=0.0219 atm AG°? H2S(g) = -34 kJ/mol SO2(g) = -300. kJ/mol H20(g) = -229 kJ/mol AG = kJ
R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".
Need help with this please ASAp\P
Dilution is done to commercially available acids such as HNO3, H,SO4 etc so that the strength is increased and so it will be safe to be used by students in a chemistry laboratory. Select one: O True O False
R = 8.314 mol-K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ - (E) · In(Q) ΔΕ. Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e 3+ (aq) + 3 e 2z (aq) 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M²+ (aq) + 2 e¯ H2 (g) + 2 OH¯ (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate A E°. cell for this galvanic cell given the reference information given at the top of the quiz. Report your answer with 3 decimal places. You do not need to report units with your answer.
AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.