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?
A reaction is found to have ΔHo = 11.4 kJ and ΔSo = 147 J/K. What...
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 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
Above what temperature in Kelvin will a reaction be spontaneous with ΔHo = 93.3 kJ and ΔSo = 152 J/K?
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.
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 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=
1. For the reaction at 298 K, P4O10s + 6H2O l → 4H3PO4s the values of ΔHo and ΔSo are -416 kJ and -209 J/K, respectively. What is the value of ΔGo at 298 K? Use correct units. ΔGo= 2. Will the following reactions show an increase or decrease for the value of ΔSrxn? NaCl s → Na+aq + Cl-aq H2O l → H2O g 2H2g + C s → CH4g 2CH3OH g + 3O2g → 2CO2g + 4H2O g
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
Compound So (J K–1 mol–1) A 42 B 58 C 88 D 16 At 298 K, ΔGo is 140 kJ for the reaction 4A + 3B → 3C + 2D Calculate ΔHo for this reaction in kJ.?
An acid–base titration was performed to determine the Ksp of a slightly soluble salt. The Ksp was experimentally determined at 53.0 oC , and the ΔGo was determined to be 25.20 kJ/mol . If ΔSo is -113 J/mol⋅K , what is ΔHo (in kJ/mol) for this slightly soluble salt? nothing kJ/mol k J / m o l