Interpretation:
The entropy
Concept Introduction:
Entropy
Kp: The equilibrium constant calculated from the partial pressures of a reaction equation. It is used to express the relationship between product pressures and reactant pressures. It is unites number, although it relates the pressures.
To find: Identify equilibrium directions for given the statement of entropy equilibrium reaction with respective images (iii).
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CHEMISTRY: ATOMS FIRST ALEKS CODE
- For the reaction conducted at 300 K below, 1.0 atm of A was placed in a chamber, and the equilibrium pressure of B was determined to be 0.4 atm. Based on this information answer the following: A (g) <---->2 B (g) If the same reaction were performed and the partial pressure of A was 0.6 atm when DG=18 kJ/mole, what would be the pressure of B? Is the reaction spontaneous in the forward or reverse direction at this point of the reaction?arrow_forwardConsider the reactionHCl(g)+ NH3(g)NH4Cl(s)Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K.ANSWER:arrow_forwardCalculatre the ΔH of reaction for the following reaction: Fe3O4 (s) + CO (g) --> 3FeO (s) + CO2 (g) ΔHfo (kJ/mol) -1118 -110.5 -272 -393.5 a -263 kJ b 54 kJ c 19 kJ d -50 kJ e 109 kJarrow_forward
- What is K if ΔG° = -20.0 kJ for a reaction at 25°? (SHOW CALCULATION)arrow_forward14 From the following ΔHo and ΔSo values predict which of reactions I, II, and III would be spontaneous at -100oC. ΔH (kJ) ΔS (J/K)I -5.0 -30II -10.0 -10III -25.0 75 Group of answer choices A, III B, I C, I and II D, II E, II and IIIarrow_forwardExplain what happens as a reaction starts with ΔG < 0 (negative) and reaches the point where ΔG = 0.arrow_forward
- Can you keep HNO3 in a Cu container? ( For a spontaneous reaction write the overall reaction)arrow_forwardWhen deltaG is positive then the reaction is____________ A) All of the above, it depends on more information B) rapidly going to products C) At equilibrium D) not going to productsarrow_forward1. A potential chemical reaction at 25.0 °C has a ΔHrxn of 147.5 kJ and a ΔSrxn of -386.9 J/K. What is the ΔGrxn in kJ. (Enter answer to 3 significant figures) Also, what is true about the potential reaction in the previous problem? a. spontaneous b. illegal c. combustive d. nonspontaneousarrow_forward
- If 2.00 mole of CsI(s) (259.81 g/mol) is placed in a 1.00 L vessel with 0.250 moles of Cs(aq)+ and 0.150 moles of I(aq)−, calculate ∆G for this reaction at 298 K (25°C) (note: R = 8.314 J/mole·K). Note, these are non-standard conditions (calculate ∆G not ∆Go)arrow_forwardWhat is ΔG°rxn for the following reaction at 298 K? SiCl4(g) + 2Mg(s) → 2MgCl2(s) + Si(s) Substance: SiCl4(g) Mg(s) MgCl2(s) Si(s) ΔG°f(kJ/mol): –616.98 0 –591.79 0arrow_forwardWhat is the sign of ΔS for the reaction Na2B4O7(s) 2 Na+(aq) + B4O72-(aq) ?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning