For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° = -113.1 kJ/mol and DS° = -145.3...
For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° =
-113.1 kJ/mol and DS° = -145.3 J/K·mol. Under which
temperature conditions would the reaction be spontaneous?
_________.
a. For all temperatures
b. Only at high temperatures
c. Only at low temperatures
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For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° =
-113.1 kJ/mol and DS° = -145.3...
2NO2(g)--2NO(g)+O2(g) (endothermic) H2(g)--2H(g) H2O(g)--H2O(l) CO2(s)--CO2(g) cem 15 Part A Predict the conditions (high temperature, low temperature,...
2NO2(g)--2NO(g)+O2(g) (endothermic)
H2(g)--2H(g)
H2O(g)--H2O(l)
CO2(s)--CO2(g)
cem 15 Part A Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous Drag the appropriate items to their respective bins. Reset Help 2NO3(e)--2NO(g) + Os(e) (endele) - 1.00 H.) - 24(e) CO.() - CO. High temperature Low temperature All temperatures No temperatures
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g)2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘for this reaction at each of the following temperatures and...
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g)2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ΔH∘ and ΔS∘ΔS∘ do not change too much within the give temperature range.) 1) 713 2) 852
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this...
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures...
Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.) ANSWER MUST BE IN kJ!! a) 722 K b) 860 K
5. Consider the following reaction: CzHs (g) → C2H4 (g) + H2 (g) AH® is +137...
5. Consider the following reaction: CzHs (g) → C2H4 (g) + H2 (g) AH® is +137 kJ/mol and AS is +120 J/K.mol. List the conditions under which this reaction is spontaneous and/or non-spontaneous. Justify your assignment (don't give exact numbers; all, high, and/or low temperature is enough)
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K...
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K...
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K The equilibrium constant for this reaction at 289.0 K is ---------- . Assume that H° and S° are independent of temperature.
calculate the deltaH given that NO2 is 33.9 kJ mol^-1 For the reaction, 7. = -114.14 kJ mol 2NO(g) + O2(g) -> 2NO...
calculate the deltaH given that NO2 is 33.9 kJ mol^-1
For the reaction, 7. = -114.14 kJ mol 2NO(g) + O2(g) -> 2NO2(g), AH Calculate AH of gaseous nitrogen that AH of NO2(g) is 33.9 kJ mol. monoxide, given
Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ...
Given the following reactions N2 (g) + O2 (g) → 2NO (g) ΔH = +180.7 kJ 2NO( g) + O2 (g) → 2NO2 (g) ΔH = -113.1 kJ the enthalpy for the decomposition of nitrogen dioxide into molecular nitrogen and oxygen 2NO2 (g) → N2 (g) + 2O2 (g) is ________ kJ.
Question number 8 The following reaction is carried out at 25o C: 2NO(g) + O2 (g)...
Question number 8 The following reaction is carried out at 25o C: 2NO(g) + O2 (g) → 2NO2 (g) These are the thermodynamic values associated with this reaction: ΔSoreaction = -147 J K-1 ΔHoreaction = -114 kJ ΔGoreaction = -70 kJ What is the effect of changing the reaction temperature to 500 K? Question 8 options: all of the answers are correct none of the answers are correct the reaction is less spontaneous at 500 K the spontaneity of the...
2NO2(g)--2NO(g)+O2(g) (endothermic)
H2(g)--2H(g)
H2O(g)--H2O(l)
CO2(s)--CO2(g)
cem 15 Part A Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous Drag the appropriate items to their respective bins. Reset Help 2NO3(e)--2NO(g) + Os(e) (endele) - 1.00 H.) - 24(e) CO.() - CO. High temperature Low temperature All temperatures No temperatures
5. Consider the following reaction: CzHs (g) → C2H4 (g) + H2 (g) AH® is +137 kJ/mol and AS is +120 J/K.mol. List the conditions under which this reaction is spontaneous and/or non-spontaneous. Justify your assignment (don't give exact numbers; all, high, and/or low temperature is enough)
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
calculate the deltaH given that NO2 is 33.9 kJ mol^-1
For the reaction, 7. = -114.14 kJ mol 2NO(g) + O2(g) -> 2NO2(g), AH Calculate AH of gaseous nitrogen that AH of NO2(g) is 33.9 kJ mol. monoxide, given
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