Making use of the provided standard enthalples in the first table below, determine standard enthalples, in kJ, for the reactions in the second table. 2Fe(s)-3CO₂(g) 3Fe₂O₂ (s) + CO(g) →→→→2Fe₂O₂ (s) + CO₂(g) Fe₂O4(s)-CO(g) 3FeO (s)-CO₂(g) Fe₂O₂ (s) + 3C0(g) - 1 2Fe(s) + 3CO₂(g) 3Fe₂O₂ (s) +9C0(g) - FeO (s)-CO(g) - Fe₂O₂ (s) + 3CO(g) 6Fe(s) +9C0₂(g) Fe(s) - CO₂(g) 1 AH-28.9 kJ ΔΗ= -37.7 kJ ΔΗ= 15.9 kJ AH= AH= AH= kj kl kj

A student dissolves 11.6 g of sodium hydroxide (NaOH)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 23.0 °C to 35.2 °C over the course of 8.9 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) Na+ (aq) + OH (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔΗ per mole of NaOH.…

A system does 566566 kJ of work and loses 216216 kJ of heat to the surroundings. What is the change in internal energy, Δ?Δ⁢E, of the system? Note that internal energy is symbolized as Δ?Δ⁢U in some sources.

A generic solid, X, has a molar mass of 58.9 g/mol. In a constant-pressure calorimeter, 30.9 g of X is dissolved in 259 g of water at 23.00 °C. X(s) · X(aq) The temperature of the resulting solution rises to 26.10 °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? q = kJ What is the enthalpy of the reaction? AH rxn kJ/mol

Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and oxygen, another method is the reaction between water and oxygen. Calculate the Δ⁢Grxn∘ of each reaction using values from the table of thermodynamic properties. (1)H2(g)+O2(g)↽−−⇀H2O2(l) Δ?∘rxn=   kJ⋅mo^l−1 (2)H2O(l)+12O2(g)↽−−⇀H2O2(l)

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction (show all work):              P4(g) + 10 Cl2(g)  →  4PCl5(s)             ΔH°rxn =  ? Given:               PCl5(s)  →  PCl3(g) + Cl2(g)                ΔH°rxn = +157 kJ              P4(g) + 6 Cl2(g)  →  4 PCl3(g)              ΔH°rxn = -1207 kJ

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* ions; that is, AH H* (aq)]=0. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S Calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits. 010

A 1.22 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/oC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.47oC to 27.95oC. What is ΔH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)

Use standard enthalpies of formation to calculate ΔH° for the following reaction: Fe2O3 (s)   +   2 Al (s)   →   Al2O3 (s)   +   2 Fe (s) Be sure to enter a unit with your answer.