Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation:2 CO (g) + 2 NO (g) → 2 CO₂ (g) + N₂ (g)AG°rxn = -689.6 kJWhat will be the Gibbs free energy change (AGrxn) in kJ if the reaction occurs at 29.28 °C? (4 sf)The partial pressures of the gases are:CO: 0.02742 atmNO: 0.02045 atmCO2: 2.469 atmN₂: 2.517 atm

2CO(g) + 2NO(g) ↔2CO2(g)+ N2 (g) Given : ∆G0 =-689.6KJ The partial pressures of the gases are PCO =…

Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation: 2 CO (g) + 2NO(g) → 2 CO₂ (g) + N₂ (8) AG rxn=-689.6 kJ What will be the Gibbs free energy change (AGrxn) in kJ if the reaction occurs at 29.28 °C? (4 sf) The partial pressures of the gases are: CO: 0.02742 atm NO: 0.02045 atm CO₂: 2.469 atm N₂: 2.517 atm

Carbon monoxide and nitrogen monoxide gases combine to form carbon dioxide and nitrogen gases according to the following balanced chemical equation: 2 CO (g) + 2NO(g) → 2 CO₂ (g) + N₂ (8) AG rxn=-689.6 kJ What will be the Gibbs free energy change (AGrxn) in kJ if the reaction occurs at 29.28 °C? (4 sf) The partial pressures of the gases are: CO: 0.02742 atm NO: 0.02045 atm CO₂: 2.469 atm N₂: 2.517 atm

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 106QRT

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When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?
The formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?
There are millions of organic compounds known, and new ones are being discovered or made at a rate of morethan 100,000 compounds per year. Organic compoundsburn readily in air at high temperatures to form carbondioxide and water. Several classes of organic compoundsare listed, with a simple example of each. Write a balanced chemical equation for the combustion in O2ofeach of these compounds, and then use the data inAppendix J to show that each reaction is product-favoredat room temperature. From these results, it is reasonable to hypothesize thatallorganic compounds are thermodynamically unstable inan oxygen atmosphere (that is, their room-temperaturereaction with O2(g) to form CO2(g) and H2O() isproduct-favored). If this hypothesis is true, how canorganic compounds exist on Earth?
Acetic acid, a weak acid, was added to a beaker containing water at 25 C, giving a solution containing molecular acetic acid, hydronium ion, and acetate ion at equilibrium. The temperature did not change. (a) Is the solution process exothermic or endothermic? (b) Was the dissolving process and partial ionization spontaneous? (c) Did the entropy of the system increase or decrease? (d) Did the entropy of the universe increase or decrease?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).
What determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?
Solid NH4NO3 is placed in a beaker containing water at 25 C. When the solid has completely dissolved, the temperature of the solution is 23.5 C. (a) Was the process exothermic or endothermic? (b) Was the process spontaneous? (c) Did the entropy of the system increase? (d) Did the entropy of the universe increase?

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