Determine the AHrxn • AH° N2(g) = 0 kJ/mol • AH°+ H2(g) = 0 kJ/mol • AH˚ NH3(g) = -46.19 kJ/mol о Example: 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 о Example: 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

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

The lattice energy is defined as the energy required to break one mole of an ionic solid into its ions in the gas phase. The lattice energy for calcium oxide corresponds to the following reaction. CaO(s) Ca2+(g) + O2-(g) DH = ? Using the following information, determine the lattice energy for calcium oxide. Ca(s) ----> Ca(g) DH = 178.2 kJ Ca(g) ----> Ca2+(g) + 2e- DH = 1747.9 kJ O2(g) ----> 2O(g) DH = 498.3 kJ O2-(g) ----> O(g) + 2e- DH = -702 kJ Ca(s) + 1⁄2 O2(g) ----> CaO(s) DH = -635.0 kJ Using the unrounded answer from the previous problem determine q (kJ) for the following reaction when 1.00 grams of solid calcium oxide forms. Ca2+(g) + O2-(g) ⟶⟶ CaO(s)
thway | Algebra. Pt Periodic Table - Pta... Scientific Calculator Gravitational Force... Conservation of Mo... Part 1-Combustion of Methane Equation for Enthalpy AH = Hbonds broken- Hsonds formed The following table is a list of selected bond energies. The bonds present in this table are common bonds for combustion reactions Selected Bond Energies Bond Energy (kI/mole) Bond Bond Energy Bond (kl/mole) H-H 436 C=0 799 O-0 495 C-C 348 O-H 463 C=C 614 C-H 413 C-C (aromatic) 519 C-O 358 N=0 623 Use the following balanced equation and chart to complete the bond energy calculations for the fuel, methane CH+202-CO2+2 H20 Compound Total Bond Energy Oxygen, O2 495 kJ/mol Carbon Dioxide, CO, 1598 kl/mol Water, H,O 926 kJ/mol
8. A substance at higher temperature always has more heat energy than a substance at lower temperature. (A) True (B) False
Using the equations H₂ (g) + Cl₂ (g) → 2 HCI (g) AH° = -184.6 kJ/mol C (s) + 2 Cl₂ (g) →→ CCI (g) AH° = -95.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction C (s) + 4 HCI (g) → CCI (g) + 2 H₂ (g). 4 2
Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC). The heat of vaporization for water in the gaseous state is 2260.0 J/g.
1. What is the enthalpy of reaction per mole of HCl (g) in the following reaction.( Don't have to explain why) 4HCl (g) + O2 (g) → 2Cl2 (g) + 2H2O + 114.4 kJ a) -457.6 kJ / mol b) -114.4 kJ / mol c) -28.6 kJ / mol d) +114.4 kJ / mol 2. The standard enthalpy of formation of a compound represents: a) The thermal energy released by the decomposition of one mole of this compound. b) The change in enthalpy when a mole of this compound is formed from its elements under standard conditions. c) The change in enthalpy when one mole of an element turns into a compound. d)The thermal energy released by the complete combustion of one mole of this compound. e) The enthalpy change of the phase transition of one mole of this compound.
CSCI has a lattice energy of -657 kJ/mol. Consider a generic salt, AB, where A²+ has the same radius as Cs*, and B has the same radius as Cl. Estimate the lattice energy of the salt AB. lattice energy of AB: kJ/mol
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 100.0 g of water at 25.0 °C, the final temperature is 37.0 °C. What is the specific heat of the alloy? The specific heat of H20(1) is 4.184 J'g-1.°c-1. q = mc AT O A. 0.423 J-g-1.°c-1 O B. 9.88 J-g-1.°C-1 O C. 48.8 J'g-1.°C-1 O D. 1.77 Jg-1.°c-1
When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1. (A) 0.397 J·g–1·°C–1. (B) 0.447 J·g–1·°C–1. (C) 1.28 J·g–1·°C–1. (D) 1.55 J·g–1·°C–1.
Question 9 of 24 Determine the enthalpy of reaction for HCI(g) + NaNO2(s) → HNO2(1) + NaCI(s) 2NACI(s) + H2O(1) → 2HCI(g) + Na20(s) AH° = -507.1 kJ/mol NO(g) + NO2(g) + Na,0(s) → 2NANO2(s) AH° = -427.0 kJ/mol NO(g) + NO2(g) → N20(g) + O2(g) AH° = -43.01 kJ/mol 2HNO2(1) → N,0(g) + O2(g) + H2O(1) AH° = +34.02 kJ/mol %3D %3D %3D Tap here or pull up for additional resources @ #3 24 & 2 8.
What will be the final temperature when a 25.0 g block of aluminum (initially at 25 °C) absorbs 10.0 kJ of heat? The specific heat of Al is 0.900 J/g· degrees C.