Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- 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'.arrow_forwardA 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 61.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy as of the first reaction, and the reaction enthalpy H 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. 4H₂O₂(1) + PbS (s) PbSO₂ (s) + 4H₂0 (1) Sn (s) + 2CO₂ (g) SnO₂ (s) + 2CO (g) ΔΗ = - 1212. kJ AS = -3559. AG = KJ Which is spontaneous? Othis reaction O the reverse reaction O neither…arrow_forwardCalculate the change in entropy for a sample heated from 298 K to 500 K under constant pressure. The constant pressure heat capacity is 29 J/mol K.arrow_forward
- In the first stage of the industrial production of nitric acid, ammonia reacts at high temperature with oxygen in a reversible, exothermic reaction: 4 NH3(g) + 5 0₂(g) 4 NO(g) + 6 H₂O(g) a) Predict the sign of the system entropy change in this reaction and explain your answer. b) Thermochemical data for this reaction are shown below. Use this data to determine the system entropy change. NH3(g) 192.3 -45.9 O₂(g) 205.0 0.0 NO(g) 210.7 90.2 H₂O(g) +188.7 -285.8 Sº / J mol-1 K-1 H₂/kJ mol-¹ c) Use the values in the table to calculate the system standard enthalpy change, AH. d) Use your answers to (b) and (c) to explain why this reaction is feasible at any temperature. e) Use your answer to (c) to calculate the surroundings entropy change in J.mol-¹ K-¹ at 298K.arrow_forwardConsider 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 remainingarrow_forwardWhat would the entropy be for a system with 6.05E+1 microstates, in J/mol-K?arrow_forward
- 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 133.0 °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. 2CH₂OH(g) + 30₂(g) → 2CO₂(g) + 4H₂O(g) 4H₂PO4(s) P4O10 (s) + 6H₂0 (1) AH-1353. kJ AS = -3331. AG = Which is spontaneous? Othis reaction O the reverse reaction Oneither ΔΗ = 439. kJ -…arrow_forwardA 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 146.0 °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.arrow_forwardfor the reaction 2NH3 - > 3H2(g) + N2(g) the equilibrium concentrations were found to be [NH3] = 0.250M, [H 2] = 0.470M and [N2] = 0.800 M. What is the equilibrium constant for this reaction?arrow_forward
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