Standard enthalpy change for a reactionEnthalpy (H) is the heat content of a system. The heat change, or enthalpy change, is represented as AH.The enthalpy change for a chemical reaction can be given asenthalpy change for the reaction = (enthalpy of formation of the products) – (enthalpy of formation of the reactants)The symbol for the standard enthalpy of reaction is AH°m, where the subscript "rxn" stands for "reaction." The standard enthalpy of a reaction is calculated from the standard enthalpy of formation values for thereactants and products.The standard enthalpy of formation is denoted as AH°e, where the subscript "f" stands for "formation." It is the enthalpy change for the formation of 1 mol of a substance in its standard state from its constituentelements in their standard states. If the standard enthalpies of formation of the reactants and of the products are known, the standard enthalpy of reaction can be calculated using the formulaAH°rxn =Eproducts nAH°t - Ereactants MAH°¢where E means sum and n and m denote the appropriate stoichiometric coefficients for each substance.Part BCalculate the standard enthalpy of the reaction, AH°Tm, for the thermite reaction:2Al(s) +Fe2O3 (s)→2FE(s) +Al½O3 (s)Elements in their standard state have an enthalpy of formation value of zero. The standard enthalpies of formation of FezOz and Al2O3 areAĦ of Fe O3(s) = -825.5 kJ/molAH of Al,O3 (s) = -1675 kJ/molExpress your answer to three significant figures and include the appropriate units.

As we know that ΔHoreaction o =∑Products nΔH0t -∑Reactant nΔH0twhere , ∑Products nΔH0t=Enthalpy…

Calculate the standard enthalpy of the reaction, AH° rn. for the thermite reaction: 2Al(s) + Fe2O3(s)→2FE(s)+ AlO3(s) Elements in their standard state have an enthalpy of formation value of zero. The standard enthalpies of formation of Fez0, and Al,0, are AH of Fe2O, (s) =-825.5 kJ/mol AH of Al,O, (s) =-1675 kJ/mol

Calculate the standard enthalpy of the reaction, AH° rn. for the thermite reaction: 2Al(s) + Fe2O3(s)→2FE(s)+ AlO3(s) Elements in their standard state have an enthalpy of formation value of zero. The standard enthalpies of formation of Fez0, and Al,0, are AH of Fe2O, (s) =-825.5 kJ/mol AH of Al,O, (s) =-1675 kJ/mol

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

How would you answer this question?
The standard enthalpy change for the following reaction is -1.55×103 kJ at 298 K. 2 Fe(s) + 10 C(s,graphite) + 5 O2(g) -> 2 Fe(CO)5(l) ΔH° = -1.55×103 kJ What is the standard enthalpy change for this reaction at 298 K?Fe(s) + 5 C(s,graphite) + 5/2 O2(g) -> Fe(CO)5(l)_______ kJ
Consider the following reaction: 2C6H6() + 15 O2(g)- 12 CO2(g) + 6 H20() AH = -5.869 x 103 kJ An unknown amount of C6H6() was combusted in a particular experiment, and the heat released from that reaction was measured to be -3.58 x 103 kJ at constant pressure. Determine the mass (in g) of O2(g) that was consumed during this experiment.
Help with the following question
Hypochlorous acid (HOCl) can decompose in the gas phase according to the following balanced equation:2 HOCl(g) ➔ 2 HCl(g) + O2(g) ΔH = -31.0 kJ (T = 298 K, P = 1 atm)Using the enthalpy of this reaction and data in the following table, calculate the standard enthalpy of formation for HOCl(g). Standard Enthalpy of Formation at 289 K Substance Formula ΔH∘f(kJ/mol)ΔHf∘(kJ/mol) Hydrogen bromide HBr(g) -36.26 Hydrogen chloride HCl(g) -92.30 Hydrogen fluoride HF(g) -268.60 Hydrogen iodide HI(g) 25.9 Methane CH4(g) -74.80 Water vapor H2O(g) -241.8
A chemist measures the enthalpy change AH during the following reaction: 2 HNO3(1) + Mg(s)→Mg (NO,),(s) + H2(g) AH=-443. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ Mg(NO,), (») + H, (g) → 2HNO, (1) + Mg(s) |kJ HNO, (1) + Mg(s) → Mg(NO,), (6) + H, (g) |kJ 2 2 2 2Mg(NO,), (s) + 2H, (g) 4HNO, (1) + 2Mg(s) |kJ
10. Compounds with carbon-carbon double bonds, such as ethylene, C,H4. add hydrogen (H,) in a reaction called hydrogenation. Calculate the enthalpy change for this reaction, using the following combustion data and Hess's Law. Overall Reaction: C,H, + H, C,H, 3C,H, + 90, 6CO, + 6H,0 ΔΗ=1401 KJ 2C,H, + 70, 4CO, + 6H,0 AH = 3500 KJ 2H, + 10, 2H,0 ΔΗ 572 KJ
The standard enthalpy change for the following reaction is 470 kJ at 298 K. 2 CH3CH,OH(g) 4 C(s,graphite) + 6 H2(g) + O2(g) AH° = 470 kJ What is the standard enthalpy change for this reaction at 298 K? 2 C(s,graphite) + 3 H2(g) + 1/2 O2(g) → CH3CH2OH(g) kJ
A scientist measures the standard enthalpy change for the following reaction to be -577.0 kJ: H,CO(g) + O2(g)–→CO{(g) + H,0(1) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H20(1) is kJ/mol.
Given the standard enthalpy changes for the following two reactions: (1) 2Pb(s) + O2(g)- →2PBO(s) AH° = -434.6 kJ (2) Pb(s) + Cl2(g) PbCl2(s) AH° = -359.4 kJ what is the standard enthalpy change for the reaction: (3) 2PBC12(s) + O2(g)2PBO(s) + 2C1½(g) AH° = ? kJ
A generic solid, X, has a molar mass of 82.3 g/mol. In a constant-pressure calorimeter, 46.1 g of X is dissolved in 337 g of water at 23.00 °C. X(s) - X(aq) The temperature of the resulting solution rises to 29.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g.°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution? 9.156 kJ Incorrect What is the enthalpy of the reaction? AHrxn 16.35 kJ/mol %D Incorrect
The standard enthalpy change for the following reaction is -479 kJ at 298 K. 2 Ni(s) + O2(g)2 NiO(s) ΔH° = -479 kJ What is the standard enthalpy change for this reaction at 298 K? Ni(s) + 1/2 O2(g) NiO(s)