Is the reaction Si(s) + 2 H2 (g) → SIH4 (g) spontaneous at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS* (universe). Compound S" (J/mol · K) A,H' (kJ/mol) Si(s) 18.82 H2 (g) 130.7 SİH4 (g) 204.65 34.31 a Calculate AS" (system), AS* (surroundings), and AS" (universe). AS" (system) = J/K AS“ (surroundings) J/K %3D AS" (universe) : J/K

Is the reaction Si(s) + 2 H2 (g) → SIH4 (g) spontaneous at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS* (universe). Compound S" (J/mol · K) A,H' (kJ/mol) Si(s) 18.82 H2 (g) 130.7 SİH4 (g) 204.65 34.31 a Calculate AS" (system), AS* (surroundings), and AS" (universe). AS" (system) = J/K AS“ (surroundings) J/K %3D AS" (universe) : J/K

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...

See similar textbooks

Similar questions

MISSED THIS? Watch IWE: Standard Enthalpies of Formation; Read Section 7.9. You can click on the Review link to access the section in your eText. Consider the table of Standard Thermodynamic Quantities for Selected Substances at 25 °C. Substance AH; (kJ/mol) Substance AH; (kJ/mol) Substance AH; (kJ/mol) Al(g) HCl(aq) NF₂ (g) Al₂O₂ (s) Cr(g) NH:(E) F(g) C(g) CH₂(g) C₂H₂(g) C₂H₂(g) C₂H6(g) CO(g) CO₂ (g) Cl(g) HCl(g) 330.0 -1675.7 716.7 -74.6 227.4 52.4 -84.68 -110.5 -393.5 121.3 -92.3 HF(g) HF (aq) H(g) Fe(g) FeO(s) Fe₂O₂ (s) Fe₂O4(s) N(g) -167.2 396.6 79.38 -273.3 -335.0 218.0 416.3 -272.0 -824.2 -1118.4 472.7 NH3(aq) O(g) O₂(g) S(g) SO₂(g) SO3(g) Sn(g) SnO(s) SnO₂ (s) -132.1 -45.9 -80.29 249.2 142.7 277.2 -296.8 -395.7 301.2 -280.7 -577.6 Part A Enter an equation for the formation of HF(g) from its elements in their standard states. Express your answer as a chemical equation including phases. Part C ΑΣΦ 6 A chemical reaction does not occur for this question. Part B Complete previous…
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)…
Determine the universe entropy change ΔS° (universe) in J/K (with 4 significant figures) for the reaction below at 298.15 K. Note that the temperature of surroundings is also 298.15 K. I2(s) + 3Cl2 (g) → 2 ICl3 (s) The standard entropy change and enthalpy change of the reaction (from the system) are given below: ΔS° (reaction) = -450.33 J/K and ΔH° (reaction) = -179.16 kJ
3.) Consider the reaction below. Reaction: AH°r (kJ/mole) 2 ICI (£) 17.78 L. (g) 247.551 l16.135 223.066 (/mole K) Which explains the outcome when 0.45 mol ½, 0.45 mol Cl2, and 2.42 mol ICl are added to a 2.0L flask at 25°C? A. [ICI] decreases B. [ICI] increases C. both [b] and [CL] increase D. at equilibrium Keywords: reaction quotient (Q), initial concentration(s), equilibrium concentration(s), equilibrium constant, forward reaction, reverse reaction, Q K. Q= K Concepts: Reaction Quotient, Chemical equilibrium
If AS at 25°C sys =-198.3 J/K, is the reaction spontaneous N2 + 3H2 → 2NH3 • AS univ = AS sys + AS surr > ? AS surr (AHsys)/T Determine the AHrxn • AH° N2(g) = 0 kJ/mol • AH° H2(g) = 0 kJ/mol • AH°; NH3(g) = -46.19 kJ/mol
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
2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7
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
Please provide full
The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)
What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C8H8(g)) = 345.2600J/mol*K and the heat of formation of C8H8(g)) is 147.8500 kJ/mol?C8H8(g) ↔ 8C(gr) + 4H2(g)a)661.88 Kb)707.958 Kc)the reaction is never spontaneousd)the reaction is always spontaneous