Part D Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) → 1 CO2(g) + 2 H2O(1) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. S° Formula J/(K-mol) CO2(g) 214 H2O(1) 189 CH4(g) 186 O2(g) 205 Express your answer with the appropriate units.

Part D Calculate the standard-state entropy for the following reaction: 1 CH4(g) + 2 O2(g) → 1 CO2(g) + 2 H2O(1) (If applicable, coefficients of one have been included for clarity.) The standard entropy values are given in the table. S° Formula J/(K-mol) CO2(g) 214 H2O(1) 189 CH4(g) 186 O2(g) 205 Express your answer with the appropriate units.

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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(Q68) Using the tabulated values from the text (located in Appendix G, beginning at p. 1211) calculate (and report in J/K) the standard entropy of reaction (AS°rxn) for the formation of gaseous nitric acid from its elements as indicated in the following balanced chemical equation: H2 (g) + N2 (g) + 3 O2 (g) --> 2 HNO3 (g)
Standard Entropy of Reaction Molecular systems tend to move spontaneously to a state of maximum randomness or disorder. Molecular randomness, or disorder, is called entropy and is denoted by the symbol S. As a state function, entropy change, A.S. depends only on initial and final states. AS has a positive value when disorder increases and a negative value when disorder decreases. The following conditions usually result in an increase in entropy: • a change of phase: solid-liquid-gas, an increase in the number of gas molecules, or • a solid dissolving to form a solution. Although the sign of the entropy change can be predicted as described above, the actual value of AS° must be calculated from the absolute entropy values. Sº, of the reactants and products: ASS° (products) - S° (reactants) ▼ Part A Predict the sign of the entropy change. AS°, for each of the reaction displayed. Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Positive Submit H₂O(1) H₂O(g)…
i need help with these pleasee Consider the reaction: 2NH3(g) +202(g) → N₂O(g) + 3H₂O(1) 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. ΔS Substance AH (kJ/mol) NH3(g) As O₂(g) 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 J/K Substance Sº (J/K mol) H₂CO(g) 219.0 0₂ (9) 205.1 CO₂(g) 213.7 H₂O(l) 69.9 SUVIL
Consider the reaction: 4HCl(g) + O₂(g) → 2H₂O(g) + 2Cl₂ (g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.69 moles of HCl(g) react at standard conditions. AS⁰ Substance So (J/K mol) HCl(g) 186.9 O2(g) 205.1 H₂O(g) 188.8 Cl₂ (g) 223.1 system = J/K
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
Consider the following reaction: 2 H2(g) + 2 NO(g) N2(g) + 2 H20(g) and the following table of standard enthalpies of formation and standard absolute entropies: compound AH (kJ mol-1) s° (J K-1 mol-1) H2(g) 130.8 NO(g) 91.3 210.8 N2(g) 191.6 H20(g) -241.8 188.8
(a) Consider the reactionCO2(g) + H2(g)→CO(g) + H2O(g)Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.70 moles of CO2(g) react at standard conditions. ∆S° surroundings=_____ J/K (b) Consider the reactionN2(g) + 2O2(g)2NO2(g)Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.40 moles of N2(g) react at standard conditions. ∆S° surroundings =____ J/K
For the following reaction (the detonation of nitroglycerin), is it spontaneous under standard conditions and how can you tell? 4 C4H5N3O9(l) (arrow >) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) ΔH = -5678 kJ
The heat of fusion AH, of acetic acid (HCH₂CO₂) is 11.7 kJ/mol. Calculate the change in entropy AS when 5.7 g of acetic acid melts at 17.0 °C. Be sure your answer contains a unit symbol. Round your answer to 2 significant digits.
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 =…
Vhemical 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 82.0 °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. 2NH, (g) N₂(g)+ 3H₂ (e) 2A1(s) + Fe₂O₂ (s) ALO, (s) + 2Fe(s) AH = 92, kJ AS = 302. FR AG = KJ Which is spontaneous? Othis reaction AS = the reverse reaction Oneither AH = -852. kJ K AG…
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…