Predict deltarH for this reaction: C2H4(g) + H2O(l) -> C2H5OH(l) using the enthalpy changes of the following reactions: C2H4(g) + 3O2(g) -> 2CO2(g) + 2 H2O(l); deltarH = -1411.1 kJ/mol-rxn C2H5OH(l) + 3O2(g) -> 2CO2 + 3 H2O(l); deltarH = -1367.5 kJ/mol-rxn Report your answer with units of kJ/mol-rxn

Calculate ΔH for the reaction; 4NH3(g) + 5O2 (g) => 4NO (g) + 6H2O (g) , from the following data. N2 (g) + O2 (g) => 2NO(g)                                  ΔH = -180.5 kJ N2 (g) + 3H2 (g) => 2NH3(g)                        ΔH = -91.8 kJ 2H2 (g) + O2 (g) => 2H2O(g)                              ΔH = -483.6 kJ Topic: Hess Law

A 0.0950 mol sample of benzoic acid (C7H6O2, MM = 122.12) was combusted in a bomb calorimeter and the temperature in the bomb calorimeter increased from 25.5ºC to 33.2ºC. Given that the heat of combustion of benzoic acid is -26.42 kJ/g, what must the calorimeter constant of this bomb calorimeter be?

(Q71) Consider the hydrogenation of ethene to form ethane that occurs according to the following balanced chemical equation: C₂H4 (g) + H₂ (8) --> C₂H6 (g). Calculate the Gibbs free energy change (in kJ) when the reaction occurs at 25°C. AHrxn= -137.5 kJ and ASrxn = -120.5 J/K.

Given the standard enthalpy changes for the following two reactions:(1) 4C(s) + 5H2(g)C4H10(g)...... ΔH° = -125.6 kJ(2) C2H2(g)2C(s) + H2(g)......ΔH° = -226.7 kJwhat is the standard enthalpy change for the reaction:(3) 2C2H2(g) + 3H2(g)C4H10(g)......ΔH° = ?

26. From the relevant bond energies given below, find the approximate AH ( in kilojoules) for the industrial synthesis of chloroform (CHC3) in a reaction of methane ( CH4) with chlorine gas (Cl2). Is the reaction exothermic or endothermic? (4 CH4 (g) + 3Cl+ (g) — СHC1(g) +3 HсI (9) Bond Dissociation Energies ( Bond Enthalpies) in kJ/mol at 298K for Selected Bonds Bond Bond Energy (kJ/mol) С —Н 410 kJ/mol Cl-Cl 243kJ/mol C-Cl 330kJ/mol H-C1 432 kJ/mol

Calculate the quantity of energy transferred (q), in kJ, by the combustion of 177 mL of acetone (C3H6O)? C3H6O(l) + 4 O2(g) → 3 CO2(l) + 3 H2O(g)        ΔHrxn = -1790 kJ Given: The density of acetone is 0.788 g/mL and its molar mass is 58.08 g/mol IMPORTANT: Enter both the sign and the value (no units), using 3 significant figures.

Given the standard enthalpy changes for the following two reactions:(1) Hg(l) + Cl2(g)HgCl2(s)...... ΔH° = -224.3 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) Hg(l) + PbCl2(s)HgCl2(s) + Pb(s)......ΔH° = ?kJ

4. Suppose 5 mL of 1.5 M ethylene diamine is added to 50 mL of 0.15 M Ni? solution in an identical calorimeter used in this experiment. The temperature rose 1.10°. Using the value for c of solution and C of the calorimeter, calculate AH for the formation of the ethylenediamine bonds. in kJ/mol.

Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) 2PbCl2(s) + O2(g)2PbO(s) + 2Cl2(g)......ΔH° = ?