Sodium reacts violently with water according to the equation: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) The resulting solution has a higher temperature than the water prior to the addition of sodium. What are the signs of AH° and AS° for this reaction? C) AH° is positive and AS° is negative. A) AH° is negative and AS° is negative. B) AH° is negative and AS° is positive. D) AH° is positive and AS is positive.

Sodium reacts violently with water according to the equation: 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) The resulting solution has a higher temperature than the water prior to the addition of sodium. What are the signs of AH° and AS° for this reaction? C) AH° is positive and AS° is negative. A) AH° is negative and AS° is negative. B) AH° is negative and AS° is positive. D) AH° is positive and AS is positive.

General Chemistry - Standalone book (MindTap Course List)

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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

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Chapter18: Thermodynamics And Equilibrium

Section: Chapter Questions

Problem 18.114QP

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Sodium reacts violently with water according to the equation: 2 Na(s) + 2 H2O) → 2 NaOH(aq) + H2g) The resulting solution has a higher temperature after the reaction. What are the signs of AH and AS° for this reaction? AH° is positive and AS° is negative. AH° is negative and AS° is positive. AH° is negative and AS° is negative. AH° is positive and AS° is positive.
The neutralization of a strong acid and strong base has an enthalpy change, ∆H°, = -55.9 kJ/mol. The net ionic equation for this reaction is H⁺(aq) + OH⁻(aq) ⇌ H₂O(l) which is the reverse of the autoionization of water, and therefore ∆H° for the autoionization of water = +55.9 kJ/mol. Kw for the autoionization of water is 1.0 × 10⁻¹⁴ at 25°C. Distilled water has a [H⁺] = 1.0 × 10⁻⁷ M and a neutral pH of 7.0. Calculate the neutral pH of distilled water at 95°C.
You may want to reference (Pages 187 - 190) Section 5.7 while completing this problem. Part A Using values from Appendix C, calculate the value of AH° for each of the following reactions. CaO(s)+ 2HC1(g)→CaCl (s) +H20(g) Express your answer using four significant figures. ΑΣφ ? AĦgm = kJ Submit Request Answer Part B 4FEO(s) + 02 (g)→2FE2O3 (s) Express your answer using four significant figures. ΔΗ kJ Submit Request Answer
Consider the following reaction at 100.0 °C: Al(s) + NaOH(aq) + H20(l) ⇄ Na[Al(OH)4](aq) + H2(g) A) Write a balanced equilibrium quotient (Qc) for the following reaction. B) If the pressure of this reaction is increased, which direction will the equilibrium shift? Why?
Ammonia reacts with water in liquid ammonia solution according to the equation: NH3(g) + H2O ⇌ NH4+ + OH− The change in enthalpy for this reaction is 21 kJ/mol, and ΔS° = −303 J/(mol·K). What is the equilibrium constant for the reaction at the boiling point of liquid ammonia (−31°C)?
Consider the ionization of nitrous acid at 25 °C: HNO2(aq) + H2O(l)H3O+(aq) + NO2–(aq) ΔG° = 19.1 kJ·mol–1What is the value of K for this equilibrium? 2.2 2.0×10–7 2.2×103 4.5×10–4
The reaction A(aq) + B(aq) C(aq) + D(aq) has a ΔHrxn = -85 kJ/mol. This reaction is endorthermic or exothermic . If the temperature of the reaction mixture is increased, equilibrium will shift towards the reactans or products. This change will decrease or increase the concentration of the reactants and K will increase or deacrease
# H₂O(1) H*(aq) + OH(aq) Calculate the pOH of a 0.0100 M HCl solution at 50.0 °C. AH = -55.8 kJ; K=1.0 x 10-¹4 (at 25.0 °C)
Item 8 Part A The value of AG" at 281.0 °C for the formation of phosphorous trichloride from its constituent elements, P2(e) + 3 Cla(e) → 2 PC (8) kJ/mol. At 25.0 °C for this reaction, AH° is –720.5 kJ/mol, AG° is 642.9 kJ/mol, and AS° is 263.7 J/K. is O 7.34 x 104 646.4 O -574.4 O - 866.6 O 1.45 x 10 Submit Request Answer
Calculate the standard enthalpy change for the reaction 4A + 2B → 2AB + A2 Given: 2A+B A2B 2A2B 2AB+ A2 AH° = – 25.0 kJ/mol %3D AH° = 35.0 kJ/mol %3D O 10.0 kJ/mol O-15.0 kJ/mol 45.0 kJ/mol -95.0 kJ/mol O-60.0 kJ/mol
Given: 2MNO(s) + O2(g) → 2MnO2(s) ArH = –269.6 kJ · mol-1
At room temperature, the equilibrium constant (Kw) for the self-ionization of water is 1.00 × 10−14. Using this information, calculate the standard free energy change for the aqueous reaction of hydrogen ion with hydroxide ionto produce water. (Hint: The reaction is the reverse of the self-ionization reaction.)

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