Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s)
DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher.
What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
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Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5...
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the reaction of dissolving silver sulfide, Ag2S, in water (25 C.) Do the calculations in two ways. Use the standard Enthalpy of formation, deltaH, and entropy S values, and the formula deltaG=deltaH-TdeltaS. Use the standard free energies of formation deltaG and the formula deltaG=deltaG(products)-deltaG(reactants).
The decomposition of calcium carbonate is given by the equation, CaCO3(s) →CaO(s) + CO2(g). Determine if the reaction is spontaneous at room temperature, given the following thermodynamics parameters: Δ? = 178 kJ/mol Δ? = 163 J/Kmol
What temperature must the reaction be above in order to become spontaneous? CaCO3(s)CaO(s)+CO2(9) AHor (CaCO3)-1207.6 k]/mol So (CaCO3) 91.7 J/mol K AHof (CaO)-35.09 kJ/mol S° (CaO) 38.2 J/mol K AHor (CO2)-393.51 kJ/mol So (CO2)213.74 J/mol K
What is K for the following reaction? CaCO3 (s) >>CO2(s) + CaO (s) Delta H=117.8kj/mol Delta S= 160.5 J/kmol Delta G=130.2jk/mol
At what temperature is the following reaction feasible: CaCO3 -> CaO + CO2? Enthalpy data: CaCO3: -1207 kJ/mol CaO: -635 kJ/mol CO2: -394 kJ/mol Entropy data: CaCO3: +93 J/K mol CaO: +40 J/K mol CO2:+214 J/K mol
CaCO3(s) ⇄ CaO(s) + CO2(g) 0.100 mol of CaCO3 and 0.100 mol CaO are placed in an 10.0 L evacuated container and heated to 385 K. When equilibrium is reached the pressure of CO2 is 0.220 atm. 0.300 atm of CO2 is added, while keeping the temperature constant and the system is allowed to reach again equilibrium. What will be the final mass of CaCO3? 7.47 g 12.54 g 18.01 g 2.00 g 10.01 g
Consider the reaction: CaCO3(s)CaO(s) + CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.26 moles of CaCO3(s) react at standard conditions. S°system = J/K
Consider the reaction CaCO3(s)Cao(s) + CO2(g The standard free energy change for this reaction is 130.4 kJ. The free energy change when 2.34 moles of CaCO (s) react at standard condition is kJ. What is the maximum amount of useful work that the reaction of 2.34 moles of CaCo,(s) is capable of producing in the surroundings under standard conditions? If no work can be done, enter none kJ Consider the reaction CaCO3(s)Cao(s) + CO2(g The standard free energy change for...
9. Consider the following reaction: inputted, <GO CaO(s) + CO2(g) - CaCO3(s); AG° = -130.9 kJ at 298 K At what partial pressure of CO2(g) will the reaction no longer be spontaneous at 298 K? (R- 0.0821 L.atm/(K.mol) = 8.31 J/(K.mol)) a. 1.59 x 108 atm b. 1.00 atm c. 6.28 x 10 atm d. 8.77 x 1022 atm e. 1.14 x 10-23 atm