Consider the reaction Fe(s) + 2HCl(aq) →FeCl₂ (8) + H₂ (9) for which AH = -7.400 kJ and AS°= 107.9 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.385 moles of Fe(s) react under standard conditions at 298.15 K. ASuniverse = J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer Retry Entire Group 5 more group attempts remaining

Consider the reaction Fe(s) + 2HCl(aq) →FeCl₂ (8) + H₂ (9) for which AH = -7.400 kJ and AS°= 107.9 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.385 moles of Fe(s) react under standard conditions at 298.15 K. ASuniverse = J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer Retry Entire Group 5 more group attempts remaining

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the reactionS(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)for which H° = -75.80 kJ and S° = -167.6 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 1.716 moles of S(s,rhombic) react under standard conditions at 298.15 K. Suniverse = J/K (2) Is this reaction reactant or product favored under standard conditions?(3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored choose 'reactant favored'.
Calculate the standard entropy of formation of liquid ethanol at 25°C. [S0(Cgraphite) = 160.70J/K•mol, S0(O2) = 205.14 J/K•mol, S0(H2) = 130.68 J/K•mol, S0(C2H5OH) = 130.68 J/K•mol]
Consider the reaction 2NH3(g) + 3N₂O(g) → 4N₂ (9) + 3H₂O(g) for which AH° = − 879.5 kJ and AS° = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.344 moles of NH3(g) react under standard conditions at 298.15 K. ASuniverse = J/K 2. Is this reaction reactant or product favored under standard conditions? 3. If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.
Consider the following reaction at 25 °C: 5 SO3(g) + 2 NH3(g) → 2 NO(g) + 5 SO2(g) + 3 H20(g) If AH° = 42.4 kJ./mol and AS° = 562.3 J/mol•K, estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature. %3D %3D
If the temperature of the surroundings is 146.55 °C, calculate the entropy change (in J/K) for the system (AS sys), surroundings (AS sur) and universe (AS universe) when 18.2 g of gaseous phenol (C6H6O) condenses. Report your answers to two decimal places. Tfus(°C) 40.90 Tvap (°C) 181.87 AH°fus (kJ/mol) 11.29 AHvap (kJ/mol) 45.69 1. AS sys Submit Answer 2. AS sur Submit Answer 3. AS universe Submit Answer Tries 0/5 Tries 0/5 Tries 0/5
Methanol is burned as fuel in some race cars. This makes it clear that the reaction is spontaneous once methanol is ignited. Yet the entropy change for the reaction 2 CH3 OH (l) + 3 O2 (g) to 2 CO2 (g) + 4 H2 O(l) is negative. Why doesn't this violate the second law of thermodynamics?
The energy produced by a spontaneous reaction is often used to provide the energy to drive nonspontaneous reactions. For example, the conversion of ATP to ADP in our cells acts as the energy source for the nonspontaneous reactions that combine amino acids during protein synthesis. Here is the conversion of ATP to ADP: ATP(aq) + H,O = ADP(aq) + HPO,²-(aq) AG° = -30.0 kj/mol A typical reaction combining two amino acids during protein synthesis has a AG = 15.0 kJ/mol. What is the minimum ATP concentration required to provide the energy to combine 1 mole of amino acid synthesis (total energy = 15.0 kJ)? Assume that the concentration of ADP = 9 µM (micromolar) and HPO42- = 4 mM (millimolar). %3! %3D
The entropy change for the processH2O(s)⟶H2O(l)is 27.9 J/K and requires that the surroundings transfer 35.0 kJ of heat to the system. Calculate the change in entropy for the universe in kJ/K at 56.2 °C.
Elemental carbon usually exists in one of two forms: graphite or diamond. It is generally believed that diamonds last forever. The table shows the standard enthalpy of formation (AH) and the standard molar entropy (Sº) values for diamond and graphite. Part A AGrxn= What is the standard Gibbs free energy for the transformation of diamond to graphite at 298 K? Cdiamond →Cgraphite Submit Express your answer to three significant figures and include the appropriate units. ► View Available Hint(s) O Substance Cgraphite Cdiamond μA Value AH (kJ/mol) Units 0 1.897 ? S° (J/mol. K) 5.740 2.38
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 144.0°C and constant total pressure. Then, he measures the reaction enthalpy ΔH and reaction entropy ∆S of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate ΔG for the first reaction and ∆S for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
What would the entropy be for a system with 6.05E+1 microstates, in J/mol-K?
Given the following reaction, calculate the standard entropy at 25oC. 2NO(g) + O2(g) 2NO2(g) (Sof NO2 = 240.1 J mol-1K-1; Sof NO = 210.8 J mol-1K-1; Sof O2 = 205.1 J mol-1K-1)