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 data,
H2(g) + 1/2 O2(g) => H2O(g) ΔGo = -240
2 H(g) + O(g) => H2O(g) ΔGo = -923
2 H(g) + 2 O(g) => H2O2(g) ΔGo = -1,070
2 O(g) => O2(g) ΔGo = -498
H2O2(l) => H2O2(g) ΔGo = 57
Determine ΔGfo for H2O2(l)
QUESTION 7 A particular reaction has a ΔHo value of -152 kJ and ΔGo of -161...
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 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?
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
QUESTION 7 A particular reaction has a ΔΗο value of-186 kJ and ΔGo of-118 kJ at 599 K. Calculate ASO at 599 K in JK 0
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
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ), ΔSo (J/K) and ΔGo(KJ) and ΔGo from the equation ΔGo ≈ ΔHo - TΔSo at 25.0 oC for 1. C2H5OH (g) → C2H4 (g) + H2O (l) 2. 2 C4H10 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (l) (Do not change a coefficient that is shown) 3. 2 C4H10 (g) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (l) (Do not change a coefficient that...
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?
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ), ΔSo (J/K) and ΔGo(KJ) and ΔGo from the equation ΔGo ≈ ΔHo - TΔSo at 25.0 oC for 1. 1 C2H5OH(g) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) (Do not change a coefficient that is shown) 2. 2 C4H10 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) (Do not change a coefficient that is shown) 3. C2H5OH (l) → C2H4 (g) + H2O (g) ...
1. Estimate the enthalpy (kJ) from bond energies CCl4(g) + O2(g) → CO2(g) + 2Cl2(g) 2. Estimate the enthalpy (kJ) from bond energies H2(g) + CO2(g) → H2O(g) + CO(g) 3. Consider the condensation reaction of CCl4. Indicate ΔSo > 0, ΔSo ~ 0, or ΔSo < 0 4. Consider the following reaction: CaCO3(s) → CaO(s) + CO2(g), Indicate if ΔSo is >0, <0, or ~0 5. Consider the condensation reaction of CCl4 and select the accurate statement, (consider signs...