Which combination of ΔHo and ΔSo will give a reaction that is nonspontaneous at all T?
ΔHo < 0; ΔSo > 0
ΔHo < 0; ΔSo < 0
ΔHo > 0; ΔSo < 0
ΔHo > 0; ΔSo > 0
Which combination of ΔHo and ΔSo will give a reaction that is nonspontaneous at all T?...
A chemical reaction has the following thermodynamic properties: ΔHo = -11.7 kJ/mol and ΔSo = -105 J/molK Determine at what temperature ( in degree celsius) the reaction becomes spontaneous, if any. Would heating make the reaction become spontaneous or nonspontaneous?
For the reaction below, ΔHo is −312.2 kJ/mol and ΔSo is −452.4 J/mol-K. 2 Cu(s) + O2(g) ⇌ 2 CuO(s) Fill in the blanks: This reaction is ___ at room temperature, and the equilibrium shifts to the ____ at higher temperatures. - at equilibrium, right - nonspontaneous, left - spontaneous, left - at equilibrium, left - spontaneous, right - nonspontaneous, right
A reaction is found to have ΔHo = 11.4 kJ and ΔSo = 147 J/K. What is the value of ΔGo at 25oC in kJ?
Above what temperature in Kelvin will a reaction be spontaneous with ΔHo = 93.3 kJ and ΔSo = 152 J/K?
QUESTION 7 A particular reaction has a ΔHo value of -152 kJ and ΔGo of -161 kJ at 484 K. Calculate ΔSo at 484 K in J/K. 1 points QUESTION 8 A particular reaction has a ΔHo value of -125 kJ and ΔSo of -230 J/mol K at 298 K. Assuming that ΔHo and ΔSohardly change with temperature, determine the temperature in K at which the spontaneity of this reaction changes. 1 points QUESTION 9 Given the following...
For the reaction at 298 K, 2NO2 g → N2O4 g the values of ΔHo and ΔSo are -58.0 kJ and -177 J/K, respectively. What is the value of ΔG nonstandard at 298 K when the concentration of N2O4 is 1.69 M and the concentration of NO2 is 2.75 M? Remember to answer in correct units. ΔG=
For the reaction: 2NO(g) + O2(g) ----> 2 NO2(g) ΔGo = −67.3 kJ and ΔSo= 146.5 J/K at 345K and 1 atm. Calculate the standard enthalpy change for the reaction of 3.75 moles of NO(g) at this temperature.Use 4 sig. figures. Hint: The ΔHo (heat absorbed or released) you have calculated is when 2 moles of NO reacted.
Suppose the ΔGof, ΔHof, and ΔSo are available and valid at 298 K. Which equation(s) would be used during the calculation of the ΔG if all product concentrations are 3 M and all reactant concentrations are 2 M and the temperature is 600 K? Choose all that apply. ΔGo= -RT ln K ΔGo=ΔHo-TΔSo ΔG=ΔGo+RT ln Q ΔGo=ΣΔGof(products)-ΣΔGof(reactants)
Consider the ribonuclease folding reaction, U → F Experimental measurements indicate the following thermodynamic parameters (T=298K): ΔGo' (kJ/mol) ΔHo' (kJ/mol) ΔSo' (J/K∙mol) -46 -280 -790 Calculate the equilibrium constants at T=298K and T=310K. K298 = ________ K310 = ________ Please show the work
Consider a reaction where E is a positive number. Is the reaction spontaneous or nonspontaneous? Which reduction potential will be higher, the anode or the cathode? a. spontaneous, anode b. spontaneous, cathode c. nonspontaneous, anode d. nonspontaneous, cathode