Nitrogen dioxide is cooled to produce dinitrogen tetroxide. Which thermochemical equation represents the reversereaction?AH°; NO2: 33.9 kJ/molAH°; N2O4: 9.2 kJ/mo2NO2(g) → 2N204(g)AH = -58.6 kJ/mol2NO2(g) → 2N204(g)AH = -24.7 kJ/molN204(1)2NO2(g)AH = 58.6 kJ/molO N204(1)> 2NO2(g)AH = 24.7 kJ/mol

Answered: Image /qna-images/answer/419fcf16-3463-437b-801a-f39c3e5ccfc2.jpg

Nitrogen dioxide is cooled to produce dinitrogen tetroxide. Which thermochemical equation represents the reverse reaction? AH NO2: 33.9 kJ/mol AH°; N204: 9.2 kJ/mo 2NO2(g) 2N204(g) AH = -58.6 kJ/mol 2NO2(g) – 2N204(g) AH = -24.7 kJ/mol N204(1) → 2NO2(g) AH = 58.6 kJ/mol N204(1) → 2NO2(g) AH = 24.7 kJ/mol

Nitrogen dioxide is cooled to produce dinitrogen tetroxide. Which thermochemical equation represents the reverse reaction? AH NO2: 33.9 kJ/mol AH°; N204: 9.2 kJ/mo 2NO2(g) 2N204(g) AH = -58.6 kJ/mol 2NO2(g) – 2N204(g) AH = -24.7 kJ/mol N204(1) → 2NO2(g) AH = 58.6 kJ/mol N204(1) → 2NO2(g) AH = 24.7 kJ/mol

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

Correct answer is d. Can you please show me how?
1. Hydrochloric acid is neutralized with potassium hydroxide in the following reaction HC1 (aq) + KOH (aq) --> KC1 (aq) + H₂O (1) DH° = -5 557 J/mol 40.00 mL of 1.500 mol/L solutions of both reactants, at 23.32 °C are mixed in a calorimeter. What is the final temperature of the mixture? Assume that the density of both solutions is 1.000 g/mL. Also assume that the specific heat capacity of both solutions is the same as the specific heat capacity of water (4.184 J/g °C).
It is recommended that the average daily intake of glucose for humans is not to exceed 32.5 g of glucose (C6H12O6). The balanced chemical equation for the combustion of glucose is shown below. C6H12O6(aq) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O (1) AH rxn= -1273.3 kJ/mol How much heat is released when 55.5 g of oxygen are combusted with glucose as shown in the reaction. above? Use the provided Periodic Table for any calculations involving elements. Report your answer to a single decimal place and report proper units with your answer.
Given the following thermochemical equations P4(s) + 6C12(g) 4PCI3(g) AH = -2439 kJ/mol 4PCI5(g) → P4(s) + 10CI 2(g) AH = 3438 kJ/mol find the AH for the reaction below, PCI5(g) → PC|3(g) + Cl2(g) O A) +249.8 kJ/mol O B) +999 kJ/mol O C) -999 kJ/mol O D) -249.8 kJ/mol
The following thermochemical equation is for the reaction of hydrogen chloride(g) with ammonia(g) to form ammonium chloride(s). HCl(g) + NH3(g) --> NH4Cl(s) ΔH = -176kJ How many grams of HCl(g) would have to react to produce 45.2 kJ of energy? _______ grams
Based on the thermochemical equation shown below, which statement is correct? C6H12O6(s) + 602(g) → 6 CO2(2) + 6H2O@) + 2803 kJ OThe reaction is exothermic and has a positive AH O The reaction is exothermic and has a negative AH O The reaction is endothermic and has a positiveH The reaction is endothermic and has a negative AH O The reaction is exothermic and has a neutral AH
The following thermochemical equation is for the reaction of carbon monoxide(g) with oxygen(g) to form carbon dioxide(g). 2CO(g) + O2(g)- →2CO2(g) AH=-566 kJ How many grams of CO(g) would have to react to produce 104 kJ of energy? grams
The combustion of a sample of isoctane vapor at constant pressure raises the temperature of a calorimeter and its contents by 0.400 °C. The heat capacity of the calorimeter and water combined is 2.48 kJ/°C. How much heat was produced from the combustion? (variations of formula: c=q/mat)
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?