Determine if the following reaction is spontaneous at 298K BaCO3(s) ↔ BaO(s) + CO2(g) ΔHf˚ = 269.3kJ/mol ΔS˚ = 171.9J/K mol

Q: For the process: Z₂(g) →2 Z(g), AH° = +478 kJ. What would be predicted for the sign of ASxn and the…

A: Given reaction: Z2(g) → 2Z(g),     ∆H∘ = +478 kJ We have to find the sign of ∆Srxn and the…

Q: Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and…

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Q: calculate the Gibbs free energy of formation of BiF5 at 298 K. Is the formation of BiF5 from the…

A: Given to us that: The formation of a BiF5 molecule by its standard elements . And Temperature T=298K…

Q: If enthalpy is +220 kJ for a reaction and entropy is +120 J, at what temperature is this…

A: The spontaniety of any reaction is decided by the Gibb's free energy change if the reaction. Any…

Q: For the reaction CO + H0 (g) - CO 2(g) + H. 2(g) , calculate the following reaction's thermodynamic…

A: Given:- CO(g) + H2O(g)-‐----------->CO2(g) + H2(g) We have to calculate Delta H° for this…

Q: The following reaction is nonspontaneous at 25°C: Cu20(s) → 2Cu(s) + '/202(g), AG° = 141 kJ/mol If…

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Q: For each reaction with ΔH = + 187 kJ/mol and ΔS = + 365 J/molK ,at what temperature at which the…

A: Given: ΔH = +187 KJ/mol or +187000 J/mol ΔS = +365 J/molK We have to calculate temperature(T) at…

Q: Describe if the following reaction is spontaneous or non-spontaneous based on enthalpy, entropy and…

A: Spontaneity of a reaction can be determined by the value Gibbs free energy.

Q: Consider the decomposition of yellow mercury (II) oxide. HgO (s,yellow) ⟶ Hg(l) + 1/2 O2(g)…

A: Given that, the decomposition of yellow mercury (II) oxide HgO (s, yellow) ⟶ Hg(l) + 12O2(g). Also,…

Q: a reaction has the following thermodynamic value of delta h =288 kj/mol and delta s =98.J/K MOL at…

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Q: Which substance would have the greatest standard molar entropy? O N2(g) NO2(g) O N2(1) O NO2(1)

A: Entropy (S): entropy dependence on randomness of a system . For example randomness order…

Q: Consider the decomposition of gaseous N2O4: N2O4(g) → 2 NO2(g) ΔH° = +57.1 kJ/mol; ΔS° = +175.8…

A: The chemical equation :  N2O4(g) ---> 2NO2(g)  ∆H° = +57.1 KJ/mol  ...or  because 1KJ = 1000 J…

Q: Explain the difference between a spontaneous and non-spontaneous process, and provide an example of…

A: Difference between spontaneous and non-spontaneous process :

Q: 9. A chemical reaction under standard state has the enthalpy of reaction: A,H° = +117 kJ and the…

A: B) The reaction is entropy driven.

Q: Place the following in order of  increasing molar entropy at 298 K.  CO,    C 5H 12 ,    H 2

A: Given CO C5H12 H2 Arrange them in order of increasing molar entropy = To be determined

Q: Above what temperature (in ºC) does the reaction with H' of 192 kJ/mol and S’ of 622 J/mol·K become…

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Q: SBr4 (g) → S (g) + 2 Br2 (l)         ΔGo = 77.75 kJ    ΔSo = 125.2 J/K    ΔHo = 115.4 kJ What would…

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Q: Consider the reaction:CO(g) + 3H2(g)CH4(g) + H2O(g)Using standard thermodynamic data at 298K,…

A: Given reaction:

Q: Directions: Calculate AG°, AH°, AS° then predict whether the reaction is spontaneous. 1. Consider…

A: The given reaction is N2 (g) + 3H2 (g) → 2NH3(g);  ΔH = - 92.4 kJ/mol Given data the absolute…

Q: Give an example for each of the following and provide an explanation.   1. A spontaneous process 2.…

A: A spontaneous process is the process which takes place on its own without any external force.

Q: Consider the following reaction at room temperature:                         Co(s) + Fe2+(aq, 1.94…

A: The above Nernst equation could be simplified as, Ecell=E°cell-0.0592VnlogQ

Q: For the reaction C2H6 (g) → C2H4 (g) + H2 (g) ΔH° is +137 kJ/mol and ΔS° is +120 J/K ∙ mol. This…

A: Given, The balanced chemical equation, C2H6 (g) → C2H4 (g) + H2 (g) ΔH°=+137 kJ = 137000 J, and ΔS°…

Q: A reaction will be spontaneous only at low temperatures if both ΔH and ΔS are negative. For a…

A: given: ∆H=-320.1KJ/mol        =-320100J/mol∆S=-95J/K.mol

Q: Using the values given for ΔH∘ and ΔS∘, calculate ΔG∘ for each of the following reactions at 298 K.…

A: Step 1: (A) For the given reaction: The value of ΔH⁰ =−844 kJ, ΔS⁰= −165 J/K, while temperature is…

Q: For a certain chemical reaction, ∆H° = -35.4 kJ and ∆S° = -85.5 J>K.Is the reaction spontaneous…

A: For a reaction is given by, ∆G=∆H - T∆S where ∆H is the heat of enthalpy, T is the temperature and…

Q: Why does the entropy of halogens at room temperature increases in the following order I2 <Br < Clz.

A: Entropy:  It is the thermodynamic property which measure molecular randomness or disorderness of a…

Q: Calculate the standard entropy change for the following reactions: Given S[So2(g)]=248.2j/k.mol,…

A: Given reaction and information,       Formation of SO3 from SO2 and O2.       Entropy value for SO2…

Q: For the process O2(g)      2O(g), ΔH° = 498 kJ·mol –1.  What would be the predicted sign of ΔS°rxn…

A: Given that :Reaction = O2(g) → 2O(g) ∆H° = 498kJ/mol

Q: For chemical reactions, the change in Gibbs free energy [at 298 K, 1at., ∆G°] determines whether a…

A: The given thermochemical equation is: C(s) + O2 (g) -----&gt; CO2 (g) ;  ∆Go = - 394 kJ For the…

Q: Can a process be spontaneous at one temperature and nonspontaneous at a different temperature?

A: Thermodynamics can be used to explain the spontaneity of a reaction.

Q: If the AH = 200 kJ/mol and AS = 133 J/K mol, at what temperature does this reaction become…

A: Given: ∆H for the reaction = 200 kJ/mol ∆S for the reaction = 133 J/K mol We have to calculate the…

Q: A chemical reaction has occurs at 308 K and has the following enthalpy and entropy changes: ΔHrxn =…

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Q: A reaction will always be spontaneous if the change in enthalpy is (positive or negative) and the…

A: Gibbs free energy is a measure of maximum reversible work that can be extracted from a system at…

Q: Under standard conditions, the products of a reaction have, overall, greater entropy than the…

A: Given that ∆S°products is greater than ∆S°reactants .

Q: Determine if this reaction is spontaneous under standard conditions; knowing that the reaction's…

A: Spontanity of reaction is determined in terms of Gibbs energy formula.

Q: 8e. Consider the following reaction: CacO3 (s) → Cao (s) + CO2 (g) Data: A,H = +177.5 kJ mol1 AS =…

A: Given: To find: The temperature of the spontaneous reaction Formula: Where is the entropy  is…

Q: Consider the following reaction; A(g) + B(g)→ c(s) + D(g); AH = -164.1 kJ; AG = 159.1 kJ at 298 K…

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Q: Place the following in order of  increasing molar entropy at 298 K.  CO  ,   C 5H 12 ,    H 2

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Q: Determine if the following reaction is spontaneous at 298K Enthalpy = -269.3kJ/Mol Entropy =…

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Q: For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would…

A: The spontaneity of the reaction can be determined by the change in Gibbs free energy. The relation…

Q: Consider the following reaction between oxides of nitrogen: NO21g2 + N2O1g2 ¡ 3 NO1g2 Calculate ∆G…

A: Standard Gibbs free energy change is given by  ∆Go=∆Ho-T∆So              ........................…

Q: Under what conditions is N2 O3(g) ⟶ NO(g) + NO2(g) spontaneous?

A: to calculate spontaneity of reaction we have the formula ∆G°298 =∆H-T∆S° where, ∆H= change in…

Q: Given the values of ΔH and ΔS, which of the following changes will be spontaneous at constant T and…

A: Given :  ΔH = 125 kJ ΔS = 15.0 J/K T = 300. K

Q: A reaction has standard DS = 50.4 J/K and standard DH = 23.7 kJ. At how many of the following…

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Q: The normal freezing point of n-octane 1C8H182 is -57 °C. In what temperature range is the freezing…

A: For freezing process  ∆H &lt; 0  and ∆S &lt; 0  So,  ∆G = ∆H - T∆S  at low temperature  ∆G &lt; 0…

Q: For the process O2(g)      2O(g), ΔH° = 498 kJ·mol –1.  What would be the predicted sign of ΔS°rxn…

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Q: At what temperatures will a reaction be spontaneous if AH = +158 kJ and AS = +411 %3D %3D J/K? O The…

A: Given ΔH = 158 kJ = 158000 J ΔS =  411 J/K

Q: 1. From the values of AH and AS, predict which of the following reactions would be spontaneous at…

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