Calculate the change in entropy for a sample heated from 298 K to 500 K under constant pressure. The constant pressure heat capacity is 29 J/mol K.

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Given, Salt: FeCl2 Mass of salt: 4.843  Mass of water: 45.1  Initial temp: 20.00  Final Temp: 32.663239    The sample of this salt is placed in water at a constant pressure calorimeter with a heat capacity of 35.5 J/℃.  Determine the enthalpy change for the dissociation of this salt, ΔHdiss.  1.    Σ qi  =  qreaction + qsolution + qcalorimeter =  0              Calculate the heat of the solution.      2. Calculate the heat of the calorimeter.   3. Calculate the heat of the reaction.   4. How many moles of your salt dissolved?   5. Calculate the value of ΔHdiss.

Trinitrotoluene (TNT) is a highly explosive compound. The thermal decomposition of TNT is described by the following chemical equation:   The enthalpy change for the explosion of ammonium nitrate with fuel oil is –7198.00 kJ for 3 moles of NH4NO3. If ΔHrxn for the thermal decomposition of 2 moles of TNT is –20,306.00 kJ, how much TNT is needed to equal the explosive power of 1 mole of ammonium nitrate?      g TNT

A2. Calculate the work done when 50 g of iron reacts with hydrochloric acid to produce FeC12(aq) and hydrogen in (a) (b) a closed vessel of fixed volume; an open beaker at 25°C. [Fe = 55.85 gmol-¹; R = 8.314 Jmol-¹K-¹]

Calculate the work w when 5.8 litre of an ideal gas at an initial pressure of 83.1 atm is expanded or compressed isothermally to a final volume of 83.1 litres reversibly. Give your answer in J.

Which of the following describes the second law of thermodynamics?deltaS(system) + deltaS (surroundings) <0deltaS (system) - deltaS (surroundings) = 0deltaS(system) - deltaS (surroundings) <0deltaS(system) - deltaS (surroundings) > 0deltaS(system) + deltaS (surroundings) = 0deltaS (system) + deltaS (surroundings) > 0

Calculate the heat of reaction at 500 K for the combustion of methane, CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) by using the date on the temperature dependence of heat capacities.