Activity 5: ANALOGY Directions: Cite an example or analogy that best interpret Enthalpy or Hess Law. EXAMPLE: Suppose you go from the first floor to the sixth floor of a building by elevator. The gain in your gravitational potential energy (which corresponds to the enthalpy change for the overall process) is the same whether you go directly there or stop at each floor on your way up (breaking the trip into a series of stens)

Activity 5: ANALOGY Directions: Cite an example or analogy that best interpret Enthalpy or Hess Law. EXAMPLE: Suppose you go from the first floor to the sixth floor of a building by elevator. The gain in your gravitational potential energy (which corresponds to the enthalpy change for the overall process) is the same whether you go directly there or stop at each floor on your way up (breaking the trip into a series of stens)

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

b My Questions | bartleby 101 Chem101 app.101edu.co Submit Question 11 of 29 In the following reaction, how much heat is generated when 3.43 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol %3D kJ 1 4 8 +/- x 100 7:50 PM O Type here to search 12/9/2019 LO
Please dear not hand written please.
a) When 3.52 g ammonia gas is oxidized over a smooth platinum catalyst to form nitrogen gas and water, 60.4 kJ of heat are released. Use this to develop a complete thermochemical equation for this process, using smallest possible whole number coefficients. b) Use the answer from part A to calculate the enthalpy change when 2 moles of nitrogen monoxide react with water from ammonia and two and a half moles of oxygen thank you so much!!
heat In an experiment, a 0.6007 g sample of nonanedioic acid (C,H1604) is burned completely sample in a bomb calorimeter. The calorimeter is surrounded by 1.085x10 g of water. During the combustion the temperature increases from 28.43 to 31.35 °C. The heat capacity of water is 4.184 J Water gloc-1 The heat capacity of the calorimeter was determined in a previous experiment to be 892.3 J/ °C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of nonanedioic acid based on these data. Insulated outside chamber Sample dish Burning sample Steel bomb > 8 H,O(1) – 9 CO,(g) C,H1604(s) - 110,(g) + Energy Combustion (bomb) calorimeter. Molar Heat of Combustion =
Direction: Use Hess' Law in determining the change in enthalpy of the chemical reaction. Follow the steps that you have learned in this module. Use a separate sheet in writing your answer. and Calculate the standard enthalpy of formation, AH° for NO23), produced from NO(g) O(g) according to the following reaction: NO(g)+ O(g) NO28) Reactions: NO() + O3 (g) NO2 (2) + O2 (g) AH° = -198.9 kJ 03 3/2 O2 (g) AH° = -142.3 kJ (g) 20 AH° = 495.0 kJ O2 (g) (g) NO NO2 (g) ΔΗ +0 (g)→ (g)
(Figure 1) Enthalpy diagram illustrating Hesa's law. The net reaction is the same as in Figure 5.21 in the textbook, but here we imagine different reactions in our two-step version. As long as we can write a series of equations that add up to the equation we need, and as long as we know a value for AHF for all intermediate reactions, we can calculate the overall AH Figure thalpy Figure Enthalpy CH₂(g) + 2O₂(g) ΔΗ, = -890 kJ AH₁ = -890 kJ AH₂=-607 kJ CO(g) + 2 H₂O(l) + O₂(g) AH. = -283 kl CH₂(g) + 2O₂(8) AH3= -283 kJ CO₂(g) + 2 H₂O(1) Part A Suppose the overall reaction wore modified to produce 2H₂O(g) rather than 2H₂O(1). Would any of the values of AH in the diagram stay the same? O yes O no Submit Provide Feedback AH₂ = -607 kJ CO(g) + 2 H₂O(1) + O₂(8) Request Answer 4 1 of 1 Next > Pr
What is the specific heat of 50.00g of a metal that raises 100.0mL of water in a calorimeter from 34.0°C to 36.09C. The initial temp of the metal was 959C. The final temp of the water and the metal is 36.0°C.
[References] Use the References to access important values if needed for this question. In the laboratory a student finds that it takes 34.1 Joules to increase the temperature of 14.2 grams of solid lead from 22.0 to 37.9 degrees Celsius. The specific heat of lead calculated from her data is | J/g°C. Submit Answer Try Another Version 10 item attempts remaining
16
Please answer all, no need for explanation I will rate your answer thank you
Ammonia reacts with oxygen as follows: 4NH3(g) + 702(g) → 4NO2(g) + 6H2O(g) AH° = -1132 kJ Calculate the enthalpy change for the formation of 3.48 mol of H2O. kJ Select the thermochemical equation for the reaction in which one mole of H20 is formed. 2/3NH3(g) + 7/602(g) → 2/3NO2(3g) + H20(g) AHº = -1132 kJ O NH3(g) + 7/4O2(g) → NO2(g) + 3/2H20(g) AH° = -283.0 kJ 4NH3(g) + 702(g) → 4NO2(g) + H20(g) AH° = -188.7 kJ O 2/3NH3(g) + 7/602(g) → 2/3NO2(g) + H2O(g) AHº = -283.0 kJ 2/3NH3(g) + 7/602(g) → 2/3NO2(g) + H2O(g) AH° = -188.7 kJ
a) How would you find the molar enthalpy (in kJ/g) for each fuel and would they compare with each other? b) what are two other factors that can be used to evaluate the fuels