Calculate the AG in kJ of the following reaction:NO₂ (g) + SO₂ (g) --> NO (g) + SO3 (8)Given the following data:AGO (NO₂) = 50.84 kJ/molAGO (SO₂) = 81.16 kJ/molAGO (NO) = -304.30 kJ/molAGO (SO3) = -377.04 kJ/molDo not put a unit in your answer.Report your answer with 1 place past the decimal point.Do not use scientific notation.

∆G for reaction = Sum of free energy of products - Sum of free energy of reactants

Calculate the AG in kJ of the following reaction: NO₂ (g) + SO₂ (g) --> NO (g) + SO3 (8) Given the following data: AGO (NO₂) = 50.84 kJ/mol AGO (SO₂) = 81.16 kJ/mol AGO (NO)=-304.30 kJ/mol AG (SO3) = -377.04 kJ/mol Do not put a unit in your answer. Report your answer with 1 place past the decimal point. Do not use scientific notation.

Calculate the AG in kJ of the following reaction: NO₂ (g) + SO₂ (g) --> NO (g) + SO3 (8) Given the following data: AGO (NO₂) = 50.84 kJ/mol AGO (SO₂) = 81.16 kJ/mol AGO (NO)=-304.30 kJ/mol AG (SO3) = -377.04 kJ/mol Do not put a unit in your answer. Report your answer with 1 place past the decimal point. Do not use scientific notation.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 12QAP: The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q,...

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The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the following steps: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) a. Use the values of Hf in Appendix 4 to calculate the value of H for each of the preceding reactions. b. Write the overall equation for the production of nitric acid by the Ostwald process by combining the preceding equations. (Water is also a product.) Is the overall reaction exothermic or endothermic?
Given the following data Ca(s)+2C(graphite)CaC2(s)H=62.8KJCa(s)+12O2(g)CaO(s)H=635.5KJCaO(s)+H2O(l)Ca(OH)2(aq)H=653.1KJC2H2(g)+52O2(g)2CO2(g)+H2O(l)H=1300.KJC(graphite)+O2(g)CO2(g)H=393.5KJ Calculate H for the reaction CaC2(s)+2H2O(l)Ca(OH)2(aq)+C2H2(g)
Consider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25C to 400C, the temperature at which the Haber process is run?
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
The thermite reaction was once used to weld rails: 2Al(s)+Fe2O3(s)Al2O3(s)+2Fe(s)(a) Using heat of formation data, calculate H for this reaction. (b) Take the specific heats of Al2O3 and Fe to be 0.77 and 0.45 J/g C, respectively. Calculate the temperature to which the products of this reaction will be raised, starting at room temperature, by the heat given off in the reaction. (c) Will the reaction produce molten iron (mpFe=1535C,Hfus=270J/g)?
Calculate H for the reaction 2NH3(g)+12O2(g)N2H4(l)+H2O(l) given the following data: 2NH3(g)+3N2O(g)4N2(g)+3H2O(l)H=1010.KJN2O(g)+3H2(g)N2H4(l)+H2O(l)H=317KJN2H4(l)+O2(g)N2(g)+2H2O(l)H=623KJH2(g)+12O2(g)H2O(l)H=286KJ
The thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?
When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?