What is the entropy change of a gas in J/K (to 2 decimal points) when one mole of a perfect gas reversibly expands from 0.36 m3 to 2.42 m3?

The heat of fusion AH, of methanol (CH,OH) is 3.16 kJ/mol. Calculate the change in entropy AS when 23. g of methanol melts at -98.0 °C. Be sure your answer contains a unit symbol. Round your answer to 2 significant digits. 0 0 X H 010

STANDARD MOLAR ENTHALPHY OR FORMATION AND REACTION: Calculate the ∆H° of the following reaction. (Use 3 decimal places for the value of ∆H°f and express your answer as well in 3 decimal places.)

Consider the combustion of propane gas:  C3H8(g)    +     5O2(g)           ------>           3CO2(g)        +            4H2O(g)            ΔHrxn  =  - 2044 kJ  Determine the sign of the entropy change for the system.

Arrange the following reactions in order of increasing ΔrxnS and briefly explain your reasoning.a) S(s) + O2(g) ⟶ SO2(g)b) H2(g) + O2(g) ⟶ H2O2(ℓ)c) CO(g) + 3 H2(g) ⟶ CH4(g) + H2O(ℓ)d) C(s) + H2O(g) ⟶ CO(g) + H2(g)

Calculate the change of the entropy of the system in J/K for the following phase transition: vaporization of 159.2 g propanol The molar mass of n-propanol (C3H7OH) is  60.095 g/mol; the enthalpy of vaporization of n-propanol is 47.5 kJ/mol; the boiling point of n-propanol is 97.7°C  Group of answer choices 128 -486 -339 1280 0.3393

3. What change will increase the entropy of the system? Group of answer choices liquid to solid solid to gas gas to liquid gas to solid 2.ΔSsyst>0 for the following reaction: Group of answer choices A,  2NO (g) + O2(g) → 2NO2(g) B, HCl (g) + NH3(g) → NH4Cl (s) C, C3H8(g) + 5 O2(g) → 3CO2 (g) + 4 H2O (g) D, 2N2 (g) + 3H2(g) → 2NH3(g) E,  Pb2+(aq) + 2Cl-(aq) → PbCl2 (s)

Suppose we redefine the standard state as P=4bar. Find the new standard ΔfG∘ values of the following substances.     Part A HCl (g)(ΔfG∘at1bar=−95.3kJmol−1)

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

Enthalpy and Gibb's Free Energy Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH₂ (products) - AH (reactants) Entropy change, AS°, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH° - TAS° where T is standard temperature, 298 K. ▼ Part A Calculate the standard enthalpy change for the reaction where the heats of formation are given in the following table: ΔΗ Substance (kJ/mol) A B C D -241 -407 191 -501 Express your answer in kilojoules. ► View Available Hint(s) {—| ΑΣΦ AHixn= 2A+B=2C+2D ? kJ…