Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**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]](https://content.bartleby.com/qna-images/question/d967ecd1-fc29-459d-be4a-b476c7e2a969/02aed317-c228-4c6c-a288-3d2a1a264f28/eb2vu_processed.jpeg)
Transcribed Image Text:**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 A
Use data from the table to predict how \( \Delta G^\circ \) for the reaction varies with increasing temperature.
- [ ] increases
- [ ] decreases
[Submit] [Request Answer]
### Part B
Calculate \( \Delta G^\circ \) 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 C
Under standard conditions is the reaction spontaneous at 600 K?
- [ ] yes
- [ ] no
[Submit] [Request Answer]](https://content.bartleby.com/qna-images/question/d967ecd1-fc29-459d-be4a-b476c7e2a969/02aed317-c228-4c6c-a288-3d2a1a264f28/fs7i6yj_processed.jpeg)
Transcribed Image Text:**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 A
Use data from the table to predict how \( \Delta G^\circ \) for the reaction varies with increasing temperature.
- [ ] increases
- [ ] decreases
[Submit] [Request Answer]
### Part B
Calculate \( \Delta G^\circ \) 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 C
Under standard conditions is the reaction spontaneous at 600 K?
- [ ] yes
- [ ] no
[Submit] [Request Answer]
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- 5.) Which of the following statements accurately describes the spontaneity of the reaction below?Al2O3(s) + 2Fe(s) → 2Al(s) + Fe2O3(s) H°rxn = 830.8 kJ/mol, S°rxn = 168 J/mol·K a. The reverse reaction is always spontaneous.b. The reaction is spontaneous above 4945 K.c. The reaction is spontaneous below 4945 K.d. The reaction is always spontaneous.e. There is not enough information to determine.arrow_forwardConsider the reaction described by the chemical equation shown. C,H,(g) + H,O(1) – C,H,OH(1) AH xn = -44.2 kJ Use the data from the table of thermodynamic properties to calculate the value of ASxn at 25.0 °C. ASixn J.K-! Calculate AGixn ·arrow_forwardFor a given reaction, ΔH = +31.15 kJ/mol and ΔS = +126.83 J/K · mol. Above what temperature is the reaction is spontaneous?arrow_forward
- 3. Calculate the value of ΔSo for the formation of POCl3 from its constituent elements, as shown below. P2(g) + O2(g) + 3Cl2(g) → 2POCl3(g)arrow_forwardCalculate AS°rxn for the following reaction. The S° for each species is shown below the reaction. N2H4(l) + H2(g) → 2 NH3(g) ings S°(J/(mol·K)) 121.2 130.7 192.8 O -59.1 J/K es O 311.0 J/K O 133.7 J/K O -133.7 J/K O 637.5 J/Karrow_forwardWhat is AS for the following reaction? 2Cl2(g) + SO2(g) SOCI₂(g) + Cl₂O(g) Substance: Cl₂(g) SO2(g) SOCI2(g) C1₂O(g) 223.0 248.1 309.8 266.1 S(J/K. mol):arrow_forward
- 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 _____Karrow_forwardCalculate AS°surr for the reaction shown below using the provided thermodynamic properties information. 2 PCI3 (g) + O2 (g) → 2 POCI3 (g) AH°f Substance (kJ/mol) PCI3 (g) -288.01 POCI3 (g) -542.2 1.706 kJ/(mol•K) 8.530 x 10-1 kJ/(mol•K) 10.17 kJ/(mol•K) 254.1 kJ/(mol•K) 20.33 kJ/(mol•K)arrow_forward
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