The neutralization of CH3COOH (aq) by NaOH(aq) (Part B) can be calculated as the sum of neutralization of H+ (aq) by OH- (aq) (Part A) and ionization of acetic acid.  Write the net ionic equations for each of these reactions and demonstrate how both of them added together yield the third one.  Using your data and Hess's law, determine the standard enthalpy of ionization of CH3COOH (aq)  Part A= Hneut= -60.006 Kj/mol

When a 2.00 g sample of KCN is dissolved in water in a calorimeter that has a total heat capacity of 1.80 kJ K-, the temperature decreases by 0.200 K. Calculate the molar heat of solution of KCN. kJ/mol AH soln

Measurements show that the energy of a mixture of gaseous reactants decreases by 305. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that -151. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? kJ exothermic O endothermic x10 X Ś 002 Ar

Given: 2MNO(s) + O2(g) → 2MnO2(s) ArH = –269.6 kJ · mol-1

When a 7.00 g sample of KCl is dissolved in water in a calorimeter that has a total heat capacity of 4.49 kJ · K-1, the temperature decreases by 0.360 K. Calculate the molar heat of solution of KCI. kJ/mol AHsoln

Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H, (g) AH = -789.0 kJ 2. HCI(g) → HCl(aq) AH2 = -74.8 kJ 3. H, (g) + Cl, (g) –→ 2 HCI(g) AH3 = -1845.0 kJ 4. MCI, (s) → MCI; (aq) AH4 = -190.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl, (g) 2 MCI,(s)

Given the reactions, X(s) + O₂(g) →→→ XO(s) XCO3(s) →→→ XO(s) + CO₂(g) what is AH for this reaction? ΔΗ X(s) + O₂(g) + CO₂(g) = ΔΗ = -651.7 kJ AH = +413.3 kJ XCO3(s) kJ

A 50.0-g sample of a copper-zinc alloy is heated to 100.0oC. The hot metal is quickly added to 100.0 g of water in a Styrofoam cup calorimeter. The initial temperature of the water is 25.00oC and the specific heat of water is 4.184 J·g–1·K–1. If the final temperature of water and alloy is 28.30oC, what is the specific heat of alloy in J·g–1·K–1?           (A) 0.276          (B) 0.385          (C) 0.697          (D) 2.09

Given these reactions, where X represents a generic metal or metalloid 1) H, (g) + 0,(g) H,O(g) ΔΗ = -241.8 kJ 2) X(s) + 2 Cl, (g) → XCl,(s) ΔΗ = +288.1 kJ 3) H,(g) + ¿Cl,(g) → HCI(g) ΔΗ -92.3 kJ 4) X(s) + O,(g) → XO,(s) AH4 = -529.5 kJ 5) Н, О(g) — н,О() H,O(1) AH5 = -44.0 kJ what is the enthalpy, AH, for this reaction? XCI, (8) + 2 H,О0() — ХО,(s)+4 HC(g) 141.62 ΔΗ kJ %3D Incorrect

A student determines the heat of dissolution of solid potassium hydroxide using a coffee-cup calorimeter of negligible heat capacity.When 0.850 g of KOH(s) is dissolved in 118.00 g of water, the temperature of the solution increases from 25.00 to 26.86 °C. Based on the student's observation, calculate the enthalpy of dissolution of KOH(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C.ΔHdissolution = ___ kJ/mol