Question

In: Chemistry

Classify the following phase changes by the signs of the system's ΔH and ΔS.

Classify the following phase changes by the signs of the system's ΔH and ΔS.

Solutions

Expert Solution

There are no systems seen in the question

However, this may help you to solve it by yourself

If ΔH is positive, it is called an endothermic reaction

If ΔH is negative, it is called an exothermic reaction.

If ΔS is positive, then it is said that randomness increased.

If ΔS is negative, then it is said that randomness decreased.

We know ΔG = ΔH - TΔS.

Enthalpy change

Entropy change

Gibbs free energy

Spontaneity

positive

positive

It depends on T, maybe + or -

yes, if the temperature is high enough

negative

positive

always negative

always spontaneous

negative

negative

It depends on T, maybe + or -

yes, if the temperature is low enough

positive

negative

always positive

never spontaneous

Dr. OWL answered 4 years ago
Next > < Previous

Related Solutions

Classify the following phase changes by the signs of the system's delta H and delta S.
Classify the following phase changes by the signs of the system's delta H and delta S.  
Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs...
Using the standard values of enthalpy changes (ΔH°) and entropy change (ΔS°) to calculate the Gibbs free energy change for the production of following metallic elements from their ore sources: (a) 2ZnO(s) 2Zn(s) + O2(g) (b) 2CaO(s) 2Ca(s) + O2(g) (c) 2Al2O3(s) 4Al(s) + 3O2(g) (d) 2MgO(s) 2Mg(s) + O2(g)
For each phase change, determine the sign of ΔH and ΔS. Sublimation , Freezing,Condensation, Deposition, Boiling , Melting
For each phase change, determine the sign of \({\Delta H}\) and \(\Delta S\) Sublimation, Freezing,Condensation, Deposition, Boiling, Melting a) \(+\Delta \mathrm{H},+\Delta \mathrm{S}\) b) \(-\Delta \mathrm{H},-\Delta \mathrm{S}\) c) \(+\Delta H,-\Delta S\) d) \(-\Delta H,+\Delta S\) Put the phase change to the correctsign of \(\Delta \mathrm{H}\) and \(\Delta \mathrm{S}\)
From the following combinations of ΔH and ΔS, predict if a process will be spontaneous at...
From the following combinations of ΔH and ΔS, predict if a process will be spontaneous at a high or low temperature: (a) both ΔH and ΔS are negative, (b) ΔH is negative and ΔSis positive, (c) both ΔH and ΔS are positive, (d) ΔH is positive and ΔS is negative.
Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn=...
Given the values of ΔH∘rxn, ΔS∘rxn, and Tbelow, determine ΔSuniv. A. ΔH∘rxn=− 118 kJ , ΔS∘rxn= 258 J/K , T= 294 K B. ΔH∘rxn= 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K C. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 294 K . D. ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 258 J/K , T= 545 K . Predict whether or not the reaction in part A will be spontaneous. Predict whether or not the reaction in part...
A) It is determined that for a particular process, ΔH = +185 kJ and ΔS =...
A) It is determined that for a particular process, ΔH = +185 kJ and ΔS = +1.80 J/K. At what temperature (in kelvin) does the reaction become spontaneous? B)Which of the following statements are true for the reaction I2(g) → 2 I(g) I. ΔH is positive II. ΔH is negative III. ΔS is positive IV. ΔS is negative V. The reaction is spontaneous at any temperature C) For which of the following processes would ΔS° be expected to be most...
Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn=...
Given the values of ΔH∘rxn , ΔS∘rxn , and T below, determine ΔSuniv . a) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 296 K Will this be spontaneous or not spontaneous? b) ΔH∘rxn= 87 kJ , ΔSrxn= 146 J/K , T= 762 K   Will this be spontaeous or not spontaneous? c) ΔH∘rxn= 87 kJ , ΔSrxn=− 146 J/K , T= 296 K   will this be spontaneous or not spontaneous? d) ΔH∘rxn=− 87 kJ , ΔSrxn= 146 J/K ,...
What are the values of  q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following constant...
What are the values of  q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following constant pressure process for a system containing 0.137 moles of CH3OH ? CH3OH(g, 122.0 ºC, 1.00 atm)  ⟶  CH3OH(l, 29.0 ºC, 1.00 atm) Assume that CH3OH(g) behaves as an ideal gas and the volume of CH3OH(l) is much less than that of CH3OH(g). Also, assume that the temperature of the surroundings is 29.0 ºC. Data: Molar heat capacity for CH3OH(g), Cp,m = 44.1 J K−1 mol−1 Molar...
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn,...
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T. (Assume that all reactants and products are in their standard states.) Part A ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer. Part B ΔH∘rxn=−84kJ, ΔS∘rxn=−157J/K, T=860K Express your answer as an integer. Part C ΔH∘rxn=84kJ, ΔS∘rxn=−157J/K, T=302K Express your answer as an integer. Part D ΔH∘rxn=−84kJ, ΔS∘rxn=157J/K, T=398K Express your answer as an integer.
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn,...
Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T. (Assume that all reactants and products are in their standard states.) Part A: ΔH∘rxn=−80.kJ, ΔS∘rxn=−154J/K, T=292K Express your answer as an integer. Part B: ΔH∘rxn=−80.kJ, ΔS∘rxn=−154J/K, T=851K Express your answer as an integer. Part C: ΔH∘rxn=80.kJ, ΔS∘rxn=−154J/K, T=292K Express your answer as an integer. Part D: ΔH∘rxn=−80.kJ, ΔS∘rxn=154J/K, T=392K Express your answer as an integer.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT