Two thermochemical equations are shown below:2Fe (s)+6H2O (1) 2Fe(OH)3 (s) + 3H2(g)AH=+322 kJ mol¹Fe2O3 (s)+3H2O (g) →2Fe(OH)3 (s) AH=+289 kJ mol¹The entropies of some chemical substances are tabulated below:Chemical speciesFe (s)O2 (g)Fe2O3 (s)Entropy (JK¹mol¹)+34.8+205+87.4It is known that chemical synthesis of one mole of iron (III) oxide from oxygenand iron achieves equilibrium at 2575 °C.Using the information provided, calculate the enthalpy of formation of water.

Step 1: 2Fe (s) + 6H2O (l) → 2Fe(OH)3 (s) + 3H2 (g)ΔH+322 kJ/molΔHf(Fe(OH)3)= ΔH / 2 = +322 kJ/mol /…

Answered: Two thermochemical equations are shown…

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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Given the reactions, X(s)+12O2(g)⟶XO(s) Δ?=−568.1 kJ XCO3(s)⟶XO(s)+CO2(g)Δ?=+128.5 kJ what is Δ? for this reaction? X(s)+12O2(g)+CO2(g)⟶XCO3(s)
Find the ΔH (in kilojoules) for the reaction below, given the following reactions and subsequent ΔH values: (Write your answer in 1 decimal place without the unit). N2(g) + 2O2(g) → 2NO 2(g) N2(g) + 3H2(g) → 2NH3(g) ΔH = -115 kJ 2NH3(g) + 4H2O(l) → 2NO2(g) + 7H2(g) ΔH = -142.5 kJ H2O(l) → H2(g) + 1/2O 2(g) ΔH = -43.7 kJ
Instant cold packs used to treat athletic injuries contain solid NH4NO3 and a pouch of water. When the pack is squeezed, the pouch breaks and the solid dissolves, lowering the temperature because of the endothermic reaction NH4NO3(s) + H₂O(1)→ NH4NO3(aq) AH = +25.7 kJ V Part A What is the final temperature in a squeezed cold pack that contains 42.5 g of NH4NO3 dissolved in 125 mL of water? Assume a specific heat of 4.18J/(g° C) for the solution, an initial temperature of 30.0 °C, and no heat transfer between the cold pack and the environment IVE ΑΣΦ 1 F O ? It = °C Submit Request Answer
None
If a system has 3.50×10^2 kcal of work done to it, and releases 5.00×10^2 kJ of heat into its surroundings, what is the change in internal energy (Δ? or Δ?)(Δ⁢E or Δ⁢U) of the system?
Choose the correct ΔH0reaction for the reaction: 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) Compound ΔH0f (kJ/mol reaction) NH3(g) -46.0 NO(g) +90.0 H2O(g) -242 A) -908 kJ/mol reactions B) -106 kJ/mol reactions C) +106 kJ/mol reactions D) -152 kJ/mol reactions E) +908 kJ/mol reactions F) +152 kJ/mol reactions
Find out the ΔH (in kJ) for the reaction: 2C(s) + H₂(g) → C₂H₂(g) Given- C(s) + O₂(g) → CO₂(g) (ΔΗ = -393.5 kJ) H₂(g) + 1/2O₂(g) → H₂O(l) (ΔΗ = -285.8 kJ) 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(I) (ΔH = -2598.8 kJ)
Given the following thermochemical reactions: N2H4() + 2H2O2(g) → N2(g) + 4H20() A) AH° = -818.3 kJ В) H2(g) + ) ½O2(g) → H20() AH° = -285.8 kJ C) H2(g) + 02(g) → H202(g) AH° = -187.8 kJ Calculate AH° of the reaction: N2H4() + O2(g) → N2(g) + 2H20() Do not encode the units. Input the final answers with 2 decimal places.
Automobile airbags contain solid sodium azide, NaN3, that reacts to produce nitrogen gas when heated, thus inflating the bag. 2 NaN3 (s) →→→ 2 Na(s) + 3 N₂(g) Calculate the value of work, w, for the system if 18.4 g NaN3 reacts completely at 1.00 atm and 22 °C. w= -1066 Incorrect J
Given the following thermochemical equations, find ΔH° for the following reaction: 2NH3(g) + 2O2(g) ⟶ N2O(g) + 3H2O(l) ΔH˚ = ? 2NH3(g) + 4SO3(g) ⟶ N2O(g) + 4SO2(g) + 3H2O(l) ΔH˚ = -290 kJ 2SO3(g) ⟶ 2SO2(g) + O2(g) ΔH˚ = 197 kJ
what is the value of ΔHrxn if the reaction below is reversed? In other words, PCl5 becomes the reactant. Report your answer in kJ to 1 decimal place. PCl3(g) + Cl2(g) → PCl5(g); ΔHrxn = 618.7 kJ
Suppose 9.44 g of calcium chloride, CaCl2, (MM=111.0 g/mol) is added to 222. g water at 21.84oC in a styrofoam cup calorimeter, and the temperature rose to 29.76oC. Calculate a value for ΔH in the equation: CaCl2(s) + H2O(l) → Ca2+(aq) + 2Cl-(aq) ΔH = ??? kJ/mol. (Assume that the styrofoam cup does not absorb any heat nor allow any heat loss; assume the specific heat of the resulting solution is 3.88 J/(goC))

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