**Part D**Calculate ΔG° at 3000 K.Express your answer in kilojoules to three significant figures.[Input Box] ΔG° = ______ kJ[Buttons: Submit, Request Answer]---**Part E**Is the reaction spontaneous under standard conditions at this temperature?[Options: - yes (radio button)- no (radio button)][Buttons: Submit, Request Answer] **Problem 19.69**Consider the following reaction between oxides of nitrogen:\[ \text{NO}_2(g) + \text{N}_2\text{O}(g) \rightarrow 3\text{NO}(g) \]The following table represents thermodynamic quantities for selected substances at 298.15 K:| Substance | \( \Delta H_f^\circ \) (kJ/mol) | \( S^\circ \) (J/(mol·K)) ||-----------|-------------------------------|--------------------------|| NO₂(g) | 33.84 | 240.45 || N₂O(g) | 81.6 | 220.0 || NO(g) | 90.37 | 210.82 |### Part AUse data from the table to predict how \( \Delta G^\circ \) for the reaction varies with increasing temperature.- [ ] increases- [ ] decreases[Submit] [Request Answer]### Part BCalculate \( \Delta G^\circ \) at 600 K, assuming that \( \Delta H^\circ \) and \( \Delta S^\circ \) do not change with temperature.Express your answer in kilojoules to three significant figures.\[ \Delta G^\circ = \][Submit] [Request Answer]### Part CUnder standard conditions is the reaction spontaneous at 600 K?- [ ] yes- [ ] no[Submit] [Request Answer]

∆G° = ∆H° - T∆S° If ∆H° = Positive, ∆S° = positive Increase in temperature increases T∆S and ∆G°…

Consider the following reaction between oxides of nitrogen: NO₂(g) + N₂O(g) →> 3NO(g) The following table represents thermodynamic quantities for selected substances at 298.15 K: AHR. Sº Substance kJ/mol J/(mol-K) NO₂(g) 33.84 N₂O(g) 81.6 NO(g) 90.37 240.45 220.0 210.62 ▼ Part A Use data from the table to predict how AG for the reaction varies with increasing temperature. O increases O decreases Submit Part B Calculate AG at 600 K, assuming that AH and AS do not change with temperature. Express your answer in kilojoules to three significant figures. AGO = Submit Part C Request Answer O yes O no ΠΙΑΣΦ 1 Request Answer → ? Under standard conditions is the reaction spontaneous at 600 K? kJ Review | Constants | Per

Consider the following reaction between oxides of nitrogen: NO₂(g) + N₂O(g) →> 3NO(g) The following table represents thermodynamic quantities for selected substances at 298.15 K: AHR. Sº Substance kJ/mol J/(mol-K) NO₂(g) 33.84 N₂O(g) 81.6 NO(g) 90.37 240.45 220.0 210.62 ▼ Part A Use data from the table to predict how AG for the reaction varies with increasing temperature. O increases O decreases Submit Part B Calculate AG at 600 K, assuming that AH and AS do not change with temperature. Express your answer in kilojoules to three significant figures. AGO = Submit Part C Request Answer O yes O no ΠΙΑΣΦ 1 Request Answer → ? Under standard conditions is the reaction spontaneous at 600 K? kJ Review | Constants | Per

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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A mixture of CO(g) and H2(g) is produced by passing steam over hot charcoal: H2O(g)+ C(s)->H2(g)+CO(g) Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound ΔGf (kJ/mol) ΔHf (kJ/mol) ΔHf (kJ/mol) H2O(g) –228.6 –241.8 188.8 H2O(ℓ) –237.2 –285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 CO(g) –137.2 –110.5 197.7 O2(g) 0.0 0.0 205.0 _____K
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