For the reaction Cr(C6H6)2 (s) --> Cr(s) + 2 C6H6 (g), the reaction internal energy change at 1 atm and 538 K is DUrxno(T = 538K) = 8.0 kJ/mol. (a) Estimate the molar enthalpy of reaction at 1 atm and 538 K for the above reaction. (b) If the standard molar enthalpy of formation for C6H6 at 1 atm and 538 K is about DHfo (C6H6 (g)) =  84 kJ/mol, estimate the standard enthalpy of formation of Cr(C6H6)2 (s) at 1 atm and 538 K.

When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…

Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).

For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 302(g)→ 2FE2O3(s) ASO = -549.73 JK1 at 298 K. The enthalpy of formation of Fe203(s) is –824.2 kJ mol. What is the standard change in Gibbs free energy for this reaction at 298 K? Item equation/constant: AG° = AHO – TASS O -660.4 kJ O -988.0 kJ O -1484.6 kJ O-1812.2 kJ