For the reaction below at 298 K: 4NO (g) → N2O (g) + N2O3 (g) ∆H = -192.7...
For the reaction below at 298 K:
4NO (g) → N2O (g) + N2O3 (g) ∆H = -192.7 kJ and ∆S = -308.2 J/K
Which of the following statements is TRUE?
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∆G > 0 at 298K |
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At higher temperatures, the reaction will be spontaneous |
||
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At lower temperatures, the reaction will be spontaneous |
||
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The reaction is spontaneous at all temperatures. |
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None of the above are true. |
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For the reaction below at 298 K:
4NO (g) → N2O (g) +
N2O3
(g) ∆H = -192.7...
QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203...
QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203 (9) AH = -192.7 kJ and AS = -308.2 J/K Which of the following statements is TRUE? AG >0 at 298K At higher temperatures, the reaction will be spontaneous At lower temperatures, the reaction will be spontAreous The reaction is spontaneous at all temperatures. None of the above are true. QUESTION 24 What is Asº at 298 K for the following reaction? 2 H2S(g)...
For the following reaction, N2 (g) + 1/2O2 (g) N2O (g) At 298 K, ΔSsurr = -...
For the following reaction, N2 (g) + 1/2O2 (g) N2O (g) At 298 K, ΔSsurr = - 275.34 J/K and ΔSsys = -74.3 J/K. Which of the following statements is true? ΔSuniv = -201.04 J/K and the process is nonspontaneous at 298K ΔSuniv = -201.04 J/K and the process is spontaneous at 298K ΔSuniv = 201.04 J/K and the process is spontaneous at 298K ΔSuniv = -349.6 J/K and the process is nonspontaneous at 298K ΔSuniv = -349.6 J/K and the process...
Enter your numbers into 1 decimal places. For the reaction: 4NO(g) + 6H2O(g) ⇋ 4NH3(g) +...
Enter your numbers into 1 decimal places. For the reaction:
4NO(g) + 6H2O(g) ⇋ 4NH3(g) +
5O2(g)
Determine ΔH° and ΔS° for the reaction at 298
K.
ΔH0(kJ)
ΔS0(J/K)
Assuming that these values are relatively independent of
temperature, calculate ΔG° at 100.°C and 2560.°C.
ΔG0(kJ)at
100℃
ΔG0(kJ)
at 2560℃
3. Is this reaction spontaneous at all range of temperature?
Enter 1 for true or 0 for false.
4. Calculate the K at 298K for the above
reaction. Enter "is" for...
1.For the reaction CH4(g) + H2O(g)3H2(g) + CO(g) H° = 206 kJ and S° = 215...
1.For the reaction
CH4(g) +
H2O(g)3H2(g)
+ CO(g)
H° =
206 kJ and S° =
215 J/K
G° for this
reaction would be negative at temperatures (above,
below) K.
For the reaction
2.2Fe(s) +
3Cl2(g)2FeCl3(s)
H° =
-799 kJ and S° =
-440 J/K
G° would be
negative at temperatures (above, below) K.
4.Consider the reaction:
NH4NO3(aq)N2O(g)
+ 2H2O(l)
Using standard absolute entropies at 298K, calculate the entropy
change for the system when 2.27
moles of NH4NO3(aq) react at
standard conditions.
S°system...
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which...
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
For the reaction: 2NO2 (g) ↔ N2O4 (g) at 298 K, The value of ∆H⁰ and...
For the reaction: 2NO2 (g) ↔ N2O4 (g) at 298 K, The value of ∆H⁰ and ∆S⁰ are -58.03 kJ and -176.6 J/K, respectively. (a) What is the value of ∆G⁰ at 298 K? (b) At what temperature would this process be spontaneous?
2NH3(g) + 3O2(g) +2CH4(g) 2HCN(g) +6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)...
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)-46193O2(g)0205CH4(g)-75186HCN(g)135.1202H2O(g)-242189The above reaction is used in the industrial production of hydrogen cyanide. (The tabulated values ?H°fand S° are for 25°C. For the purposes of this question assume that ?H° and ?S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)?H° is -939.8?S° is 165Calculate ?G° at 1005°C, for this equation.Are the following statements about this process True...
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN....
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN. Compute K for this reaction. a) 1.01 Ob) 0.998 O c) 0.948 O d) 6.89 Oe) 10.23
Need serious help on these 3! Please help! Which of the following should have the largest...
Need serious help on these 3! Please help!
Which of the following should have the largest value of S degree? a) SF_6 (g) at 298K b) H_2O (l) at 298K c) He(g) at 298K d) CH_3OH (l) at 298K Which of these changes in the distribution of the nine particles shows an decrease in entropy? Which of these statements is true for this reaction? FeO(s) + CO(g) rightarrow CO_2(g) + Fe(s) Delta H = -11.0 kJ; Delta S = -17.4...
Enter your numbers into 1 decimal places; Enter "is" for infinitely small and "ig" infinitely great; For the reaction:...
Enter your numbers into 1 decimal places; Enter "is" for infinitely small and "ig" infinitely great; For the reaction: 4NH3(g)502(g) 4NO(g)6H20(g) 1. Determine AH° and AS° for the reaction at 298 K. AH°(kJ) ASU/K) 2. Assuming that these values are relatively independent of temperature, calculate AGo at 100.°C 2560. C, and 3540. C. AG°(kJ) at 100°C AGO(kJ) at 2560°C 3. Is this reaction spontaneous at all range of temperature? Enter 1 for true or 0 for false. 4. Calculate the...
QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203 (9) AH = -192.7 kJ and AS = -308.2 J/K Which of the following statements is TRUE? AG >0 at 298K At higher temperatures, the reaction will be spontaneous At lower temperatures, the reaction will be spontAreous The reaction is spontaneous at all temperatures. None of the above are true. QUESTION 24 What is Asº at 298 K for the following reaction? 2 H2S(g)...
Enter your numbers into 1 decimal places. For the reaction:
4NO(g) + 6H2O(g) ⇋ 4NH3(g) +
5O2(g)
Determine ΔH° and ΔS° for the reaction at 298
K.
ΔH0(kJ)
ΔS0(J/K)
Assuming that these values are relatively independent of
temperature, calculate ΔG° at 100.°C and 2560.°C.
ΔG0(kJ)at
100℃
ΔG0(kJ)
at 2560℃
3. Is this reaction spontaneous at all range of temperature?
Enter 1 for true or 0 for false.
4. Calculate the K at 298K for the above
reaction. Enter "is" for...
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN. Compute K for this reaction. a) 1.01 Ob) 0.998 O c) 0.948 O d) 6.89 Oe) 10.23
Need serious help on these 3! Please help!
Which of the following should have the largest value of S degree? a) SF_6 (g) at 298K b) H_2O (l) at 298K c) He(g) at 298K d) CH_3OH (l) at 298K Which of these changes in the distribution of the nine particles shows an decrease in entropy? Which of these statements is true for this reaction? FeO(s) + CO(g) rightarrow CO_2(g) + Fe(s) Delta H = -11.0 kJ; Delta S = -17.4...
Enter your numbers into 1 decimal places; Enter "is" for infinitely small and "ig" infinitely great; For the reaction: 4NH3(g)502(g) 4NO(g)6H20(g) 1. Determine AH° and AS° for the reaction at 298 K. AH°(kJ) ASU/K) 2. Assuming that these values are relatively independent of temperature, calculate AGo at 100.°C 2560. C, and 3540. C. AG°(kJ) at 100°C AGO(kJ) at 2560°C 3. Is this reaction spontaneous at all range of temperature? Enter 1 for true or 0 for false. 4. Calculate the...
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