Question

In: Chemistry

For the following half reaction: N2(g) + 5H+(aq)+4e- ----> N2H5+ Calculate the amount of time required...

For the following half reaction: N₂(g) + 5H⁺(aq)+4e^- ----> N₂H₅⁺

Calculate the amount of time required to produce 7.86 (g) of N₂ while using a 15.0 A current.

Expert Solution

weight (W) = 7.86

current (i) = 15 A

faraday (F) = 96500 C

N2 -------------------> N2H5+

0 -2 --------------------> oxidation state of N atom

for 2 N atoms change is oxidation state = -4 (4 units)

equivalence weight of N2 (E) = molecular weight / valency

= 28 /4

= 7 GEW

from faraday law

W = E x i x t / 96500

7.86 = 7 x 15 x t / 96,500

t = 7223.7 sec

t = 120.39 min

time required = t = 7223.7 sec = 120.39 min

queen_honey_blossom answered 2 months ago

answer both pls 1. Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- → 2H2O(l) Eo...

answer both pls 1. Consider the following half-reaction. 4H+(aq) + O2(g) + 4e- → 2H2O(l) Eo = 1.23 V What is E, if the pressure of oxygen gas is 1.0 atmosphere and the pH is 2.92? USE 2 DECIMAL PLACES. (Hint, are solids and pure liquids included in Q? Using LeChatelier's principle is E going to be larger or smaller?) 2. Mg2C2O4(s) → 2Mg2+(aq) +C2O42-(aq) Ksp = 8.6 x 10-5 What is Qsp if 100 mL of 0.080 M Mg(N03)2...

The standard half-cell potential for the reaction O2(g)+4H+(aq)+4e−→2H2O(l) is +1.229 V at 298.15 K. The aO2...

The standard half-cell potential for the reaction O2(g)+4H+(aq)+4e−→2H2O(l) is +1.229 V at 298.15 K. The aO2 = 1.00 assuming that the aH+ is equal to the molality. Part A Calculate E for a 0.100-molal solution of H2SO4 for aO2 = 1.00 assuming that the aH+ is equal to the molality. Part B Calculate E for a 0.100-molal solution of H2SO4 for aO2= 1.00 using the measured mean ionic activity coefficient for this concentration from the data tables in the textbook....

For the following reaction, the concentration of A and the amount of time required to decrease...

For the following reaction, the concentration of A and the amount of time required to decrease that concentration to one-half of the initial concentration, t1/2, are directly proportional. Therefore, a decrease in concentration of A shows a proportional decrease in the half life, t1/2. What is the order of this reaction? If the rate constant for this reaction is 0.0355 M·s–1 at 400 °C, what is the half-life of this reaction, given an initial concentration of 0.569 M.

Consider the half-reaction below (in an acidic solution). NO3??(aq) ? NO(g) Which of the following is...

Consider the half-reaction below (in an acidic solution). NO3??(aq) ? NO(g) Which of the following is needed to balance this half-reaction? A) 3e?? are needed on the reactants side. B) 4H?+ are needed on the reactants side. C) 2 H2O are needed on the products side. D) All of these are needed to balance the given reaction.

write cell half chemical reaction and global reaction: PblPbSO4lSO42-llCu2+(aq)lCu PtlTI+(aq),TI3+(aq)llCu2+(aq)lCu CdlCdCl2llHNO3(aq), H2lPl PtlH2(g)lHCl (aq)lCl2lPl calculate delta...

write cell half chemical reaction and global reaction: PblPbSO4lSO42-llCu2+(aq)lCu PtlTI+(aq),TI3+(aq)llCu2+(aq)lCu CdlCdCl2llHNO3(aq), H2lPl PtlH2(g)lHCl (aq)lCl2lPl calculate delta G and Ks

The half-life of a reaction, t1/2, is the time required for one-half of a reactant to...

The half-life of a reaction, t1/2, is the time required for one-half of a reactant to be consumed. It is the time during which the amount of reactant or its concentration decreases to one-half of its initial value.Determine the half-life for the reaction in Part B using the integrated rate law, given that the initial concentration is 1.95 mol⋅L−1 and the rate constant is 0.0019 mol⋅L−1⋅s−1

The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq)...

The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq) is 86.6 s at 25.0oC and its half-life is 66.2 s at 45.0oC. What is its half-life (in s) at 65.0oC?

a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V

13)) a) Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e- 2F-(aq) 2.870V 2H+(aq) + 2e- H2(g) 0.000V Zn2+(aq) + 2e- Zn(s) -0.763V (1) The weakest oxidizing agent is: enter formula (2) The strongest reducing agent is: (3) The strongest oxidizing agent is: (4) The weakest reducing agent is: (5) Will F-(aq) reduce Zn2+(aq) to Zn(s)? (6) Which species can be reduced by H2(g)? If none, leave box blank. b)) Consider the following half-reactions: Half-reaction E° (V) Ag+(aq) +...

25. The half-reaction at the anode for the following balanced reaction is: 3MnO4 - (aq) +...

25. The half-reaction at the anode for the following balanced reaction is: 3MnO4 - (aq) + 5Fe (s) + 24H+ (aq) ¬ 5Fe+3 (aq) + 3Mn+2 (aq) + 12H2O (l) a. Fe+2 (aq) → Fe+3 (aq) + e - b. MnO4 - (aq) + 8H+ (aq) + 5 e - → Mn+2 (aq) + 4H2O (l) c. Fe (s) → Fe+3 (aq) + 3 e - d. 2MnO4 - (aq) + 12H+ (aq) + 6e→ 2Mn+2 (aq) + 3H2O (l)

Calculate the values of Delta G and Ecell for the following reaction, label the half reactions...

Calculate the values of Delta G and Ecell for the following reaction, label the half reactions as anode and cathode. 2Ag(s) + Cu2+ (aq) > 2 Ag+ (aq) + Cu(s) * My main question lies in which is cathode and anode...it seems that the Ag half reaction (2Ag(s) > 2Ag+ +2e-) signifies Ag(s) loosing electrons causing the positive reactant, this leads me to think loss of electrons/this is the oxidation half reaction, therefore Ag(s) is the reduction agent and anode...