Consider the data in the table. Compound Melting point (°C) AHfus (kJ/mol) Boiling point (°C) AHyap (kJ/mol) HF -83.11 4.577 19.54 25.18 НСІ 1.991 -84.9 17.53 -114.3 HBr -86.96 2.406 -67.0 19.27 -35.38 HI -50.91 2.871 21.16 Using the data in the table, calculate A.Sfus and ASvap for HF. 24.08 J/(K mol) J/(K mol) 86.03 ASfus ASvap = Determine the entropy change when 2.50 mol HF(g) condenses at atmospheric pressure. AS J/K

Select the correct statement or relationship. A negative Gibbs energy, corresponds to a spontaneous reaction or process. O A positive Gibbs energy, corresponds to a spontaneous reaction or process. O A negative Gibbs energy, corresponds to a nonspontaneous reaction or process. O All the statements here are incorrect.

For a certain reaction changeH֯ =-83.5 kJ and changeSͦ =-148 j/K. If the values of changeH֯ and changeSͦ can be assumed to be constant for all temperatures, the temperature at which the reaction is at equilibrium is?

The standard Gibbs free energy, ∆??, is:a) The residual energy present in the reactants in the equilibrium stateb) The residual energy present in the products in the equilibrium statec) The difference in the residual energy of the reactants and products inBalance.d) The energy required to convert one mole of reactants into one mole ofproducts[justify the answer you consider correct]

A Moving to another question will save this response. Question 11 A reaction has an equilibrium constant (K) of 58.2. If the entropy of this reaction is-36.7 J/mol"K at a temperature of 317 K, what is the enthalpy of this reaction in kJ/mol? Report your answer to one decimal place. If your answer is negative, make sure to input a negative sign (-). Moving to another question wvill save this response. lyp 144 &

Which of the givenn processes will cause a decrease in entropy? Note only one is correct. - dissolving NaCl in water? - removing a partition to mix two gases? - freezing water to make ice? - boiling water to make steam? - heating ice to make water?

REFER TO IMAGE

The following reaction is endothermic: H₂(g) + 12(g) → 2HI(g) K= 5.0x10¹ at 400°C

The entropy of any substance at any temperature above absolute zero is called the: Select the correct answer below:   absolute entropy   standard entropy   free entropy   none of the above

At 0.9 bar of pressure and 373.15 K, the hypothetical transition from liquid to gaseous water will result in what change in the total entropy of the “universe”? No change An increase in the total entropy A decrease in the total entropy Not enough information to determine