Ammonia is an important chemical for fertilizer production around the world. One method to produce ammonia is by the electrochemical reaction between water and nitrogen using a reverse fuel cell. A simplified reaction proceeds as: 2N2 + 6H20 --> 302 + 4NH3 What volume of ammonia gas at 55°C and 580 mmHg will be produced from 2.00 g of nitrogen? Assume ammonia is an ideal gas. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).

Ammonia is an important chemical for fertilizer production around the world. One method to produce ammonia is by the electrochemical reaction between water and nitrogen using a reverse fuel cell. A simplified reaction proceeds as: 2N2 + 6H20 --> 302 + 4NH3 What volume of ammonia gas at 55°C and 580 mmHg will be produced from 2.00 g of nitrogen? Assume ammonia is an ideal gas. For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac).

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...

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B through D please. Thanks!
Given the following half-reactions: AIF6 + 3e- Al + 6F A13+ + 3e Al E = -2.07 V %3D E = -1.66 V %3D Calculate the equilibrium constant at 25°C for the reaction 3- A1$+ (aq) + 6F(aq) AIF6 (aq) (Enter your answer to two significant figures.) K
The electrochemical reaction which powers a lead-acid storage battery is as follows: Pb(s) + PbO2(s) + 4H*(aq) + 2SO,²-(aq) → 2PBSO4(s) + 2H20(1) A single cell of this battery consists of a Pb electrode and a PbO2 electrode, each submerged in sulfuric acid. What reaction occurs at the cathode during discharge? O PbO2(s) is oxidized to PbSO4(s). O PbO2(s) is reduced to PbSO4(s). H* is oxidized to H20(1) . O Pb(s) is oxidized to PbSO4(s). O Pb(s) is reduced to PbSO4(s).
Part A Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag*(aq) +e –→ Ag(s) What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for 78 min? Express your answer to two significant figures and include the appropriate units. Value Units m = Submit Request Answer
www-awu.aleks.com/ 18.3 Gibbs Free E... M 5.3 Enthalpies of... O ELECTROCHEMISTRY Writing the half-reactions of a single-displacement reaction Study this chemical reaction: oxidation: 2 AgNO3(aq) + Cu(s) 2 Ag(s) + Cu(NO3)₂(aq) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. reduction: Explanation 18.5 Gibbs Free E... Chec 5 ローロ e > X C 0° Reading Schedule 19.6 Reduction Po S e tv Is C 2022 McGraw Hill LLC
true or false Doubling the stoichiometric coefficients in a chemical reaction will square the value of the equilibrium constant (K), will double ΔG°, and will not change E°.
Be sure to answer all parts. How many faradays of electricity are required to produce (a) 0.93 L of 02 at exactly 1 atm and 25°C from aqueous H2SO, solution? faradays (b) 9.08 L of Ch at 750 mm Hg and 20°C from molten NaCl? faradays (c) 8.0 g of Sn from molten SnCl? faradays
3:19 PM Thu May 4 * 8 J ↑ M ● ( 9 K 8 H x H₂O O O 9 L cmd = (aq) P H3O+ "' X 0 : ; { [ 300 option ? 1 50 69% Ï Submit 1 delete 1
Experimental solid-oxide fuel cells that use butane (C4H10C4H10) as the fuel have been reported recently. These cells contain composite metal/metal oxide electrodes and a solid metal oxide electrolyte. The cell half- reactions are Anode:C4H10(g)+13O2- (s)→4CO2(g)+5H2O(1)+26e-Cathode:02 (g)+4e-→202-(s) a) calculate the value of E• for the cell reaction at 25 °C b) calculate the value of the pK=-log(K) for the cell reaction at 25 °C (K is the equilibrium constant of the reaction) C) How many grams of butane are required to produce a constant current of 10.2 A for 7.40 h ? d)How many liters of butane at 20 °C and 788 mmHg pressure are required?
As the cell reaction within an automobile lead storage battery proceeds, the sulfuric acid is consumed: Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4– → 2PbSO4(s) + 2H2O(l) Eocell = 2.043 V Thus the H2SO4 concentration of the solution within the battery goes down over time. Calculate (a) the reaction quotient and (b) the nonstandard cell potential of a lead storage battery at 25oC when the molar concentration of sulfuric acid is 0.25 M. [Consider H2SO4(aq) to be 100% dissociated into H+(aq) and SO42-(aq) when you calculate Q.] Show your work and explain why your answers make sense in terms of what you know about 12 V batteries.
Fill in the following brackets: Redox reactions can also lead to greenhouse gas emissions from soils. Under very strongly reducing conditions (Eh < -0.1) the dominant GHG released from soils is likely ["carbon dioxide", or "methane", or "nitrous oxide", or "nitrous oxide and carbon dioxide"], whereas, at oxidizing conditions (Eh > +0.2) release of ["carbon dioxide", or "methane", or "nitrous oxide", or "nitrous oxide and carbon dioxide"] is more favorable.
Part A Silver can be electroplated at the cathode of an electrolysis cell by the half-reaction: Ag (aq) + e¯→ Ag(s) What mass of silver would plate onto the cathode if a current of 8.1 A flowed through the cell for 63 min ? Express your answer to two significant figures and include the appropriate units. Templates Symbols uado redo resat keyboard shortcuts help, Value Units m =