1.) 2.) 3.) 4.) The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O

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The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) rightarrow 2 CO2(g) + 3 H2O(I) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction, reaction (1): C(s) + O2(g) rightarrow CO2(g) Delta H = -393.5 kJ/mol reaction (2): H2(G) + 1/2 02(g) rightarrow H20(I) DELATH = -285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) rightarrow C2H6(g) DELTA H = -84.0 kJ/mol KJ/mol Calculate the standard enthalpy change (Delta H Deg rxn) for the reaction of Fe2O3(s) and CO(g) to form Fe3O4(s) and CO2(g) given the standard enthalpies of formation (Delta H Deg f) shown in the table below. (Include the sign of the value in your answer.) When a chemist mixed 2.45 g of NaOH and 5.81 ml_ of 0.63 M HCI in a constant-pressure calorimeter, the final temperature of the mixture was 23.8 degree C. Both the HCl and NaOH had the same initial temperature, 20.9 degree C. The equation for this neutralization reaction is: NaOH(s) + HCl(aq) rightarrow NaCl(aq) + H2O(J). Given that the density of each solution is 1.00 g/mL and the specific heat of the final solution is 4.1801 J/g.K, calculate the enthalpy change for this reaction in kJ/mol NaOH. Assume no heat is lost to the surroundings. KJ/mol NaOH In a coffee-cup calorimeter, 1.62 g KOH is added to 125 ml of 0.80 M HCI. The following reaction occurs. KOH(s) + HCl(aq) rightarrow H2O(J) + KCl(aq) Due to the reaction, the temperature of the solution changes from 32.8 degree C to 39.0 degree C. Given that the density of the HCl solution is 1.00 g/ml, and the specific heat of the final solution is 4.18 J/g*K, calculate the enthalpy change for this reaction in kJ/mol KOH. KJ/mol

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