Consider the reaction: 2NH3 (9) +202(g) → N₂O(g) + 3H₂O(l) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.64 moles of NH3(g) react at standard conditions. AS Substance AH (kJ/mol) NH3(g) 0₂ (9) AS N₂O(g) H₂O(1) surroundings Consider the reaction: system -46.1 0.0 82.1 -285.8 H₂CO(g) + O₂(g) → CO₂(g) + H₂O(1) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.63 moles of H₂CO(g) react at standard conditions. J/K 3/K Substance S (J/K mol) H₂CO(g) 219.0 0₂ (9) 205.1 CO₂(g) 213.7 H₂O(1) 69.9 YUSSUIVIE

Consider the reaction: 2NH3 (9) +202(g) → N₂O(g) + 3H₂O(l) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.64 moles of NH3(g) react at standard conditions. AS Substance AH (kJ/mol) NH3(g) 0₂ (9) AS N₂O(g) H₂O(1) surroundings Consider the reaction: system -46.1 0.0 82.1 -285.8 H₂CO(g) + O₂(g) → CO₂(g) + H₂O(1) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.63 moles of H₂CO(g) react at standard conditions. J/K 3/K Substance S (J/K mol) H₂CO(g) 219.0 0₂ (9) 205.1 CO₂(g) 213.7 H₂O(1) 69.9 YUSSUIVIE

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 reaction: 2Na(s) + 2H₂O(1) → 2NaOH(aq) + H₂(g) Using standard thermodynamic data at 298 K, calculate the entropy change for the surroundings when 1.55 moles of Na(s) react at standard conditions. ASO Substance AH (kJ/mol) Na(s) H₂O(1) NaOH(aq) H₂(g) surroundings = 0.0 -285.8 -470.1 0.0 J/K
Round everthing to 4 decimal places. Ammonia and carbon dioxide are produced from the hydrolysis of urea, the corresponding chemical reaction shown below:
Using the provided data, determine the temperatures at which the following hypothetical reaction will be spontaneous under standard conditionsA + B → 2C + D△S°rxn = 249.1 J/K△H°rxn = 104.6 kJ * at no temperatures * at all temperatures below 146.9 °C * at all temperatures above 146.9 °C * at all temperatures above 238.1 °C * at all temperatures below 238.1 °C * at all temperatures
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) → ADP(aq) + HPO (aq) for which AGixn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.40 mM, and [HPO?-] = 5.0 mM. AGxn kJ/mol %3D Is the hydrolysis of ATP spontaneous under these conditions? O yes
Calculate the standard molar entropy of vaporization of water at 57.0 °C, given that its standard molar entropy of vaporization at 100.0 °C is 109.0 J-K-¹ mol-¹ and the molar heat capacities at constant pressure for liquid water and water vapor are 75.3 J-K-¹.mol-¹ and 33.6 J-K-¹.mol-¹, respectively, in this temperature range. AS vap 103.7 Incorrect J. K-1 mol-1 A
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.
Consider the reaction Fe(s) + 2HCl(aq) → FeCl₂ (s) + H₂(g) 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
0/5 Nerbs A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 85.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS 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. do AH = -2220. kJ J AS = -6189 K C,H, (g) + 50, (g) 3Co, (g) + 4H,0(1) AG = KJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -50. kJ 0- AS =…
A chemicai 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 42.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS 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. ΔΗ Ξ - 70. kJ J AS = -151. K TiCl, (g) + 2H,0(g) → Tio, (s) + 4H Cl (g) AG = || kJ Which is spontaneous? this reaction the reverse reaction neither AH = 439. kJ AS = K 4H,PO, (s) →…
Enthalpy and Gibb's Free Energy Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH₂ (products) - AH (reactants) Entropy change, AS°, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH° - TAS° where T is standard temperature, 298 K. ▼ Part A Calculate the standard enthalpy change for the reaction where the heats of formation are given in the following table: ΔΗ Substance (kJ/mol) A B C D -241 -407 191 -501 Express your answer in kilojoules. ► View Available Hint(s) {—| ΑΣΦ AHixn= 2A+B=2C+2D ? kJ…