At 298 K, for the reaction
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- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forwardPredict whether each reaction is reactant-favored or product-favored at 298 K and 1 bar, and calculate the minimum work that would have to be done to force it to occur, or the maximum work that could be done by the reaction. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)arrow_forward
- Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?arrow_forwardWhich of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_forwardConsider planet Earth as a thermodynamic system. Is Earth thermodynamically or kinetically stable? Discuss your choice, providing as many arguments as you can tosupport it.arrow_forward
- Calculate the standard reaction entropy for N2(g) + 3 H2(g) → 2 NH3(g) at 25 °C. (b) What is the change in entropy when 2 mol H2 reacts?arrow_forwardCalculate ΔS (for the system) when the state of 2.00 mol of gas molecules, for which Cp,m = R, is changed from 25 °C and 1.50 atm to 135 °C and 7.00 atm.arrow_forwardCalculate the change in internal energy (in kcal) for the reaction Cl₂(g) +7/2O2(g) = Cl₂O(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O(g) is 63.4 kcal mol-¹ at 25 °C.arrow_forward
- Calculate the change in internal energy (in kcal) for the reaction Cl2(g) + 7/2 O2(g) = Cl₂O7(g) at 25 °C, given that the gases are ideal. The enthalpy, AH, for the formation of Cl₂O7(g) is 63.4 kcal mol- ¹ at 25 °C.arrow_forwardA closed, but not isolated system is in thermal contact with its surroundings. The system's volume is fixed at 7.3 L. Both the system and surrounds have a temperature of 25 °C. A chemical reaction occurs inside the system for which ΔrU = 11.38 KJ. (A) What is the change in entropy for the surroundings for the process, ΔSsurr? (B) What are the ranges of possible values for the change in entropy of the system, ΔSsys , for this process?arrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?arrow_forward
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