Calculate the work (w) and ΔEo, in kJ, at 298 K and 1 atm pressure, for the combustion of one mole of C6H6 (g). First write and balance the equation. The products will be CO2 (g) and H2O (g). The value of ΔHo for this reaction is -3169.3 kJ/mol.  The value for w in kJ =  The value for ΔEo ( in kJ) =

One day while camping, a student used a propane stove to boil some water. The student heated 5.00 L of water from 15.6°C to 98.5°C. The molar enthalpy of combustion of propane is -2043.9 kJ/mol and heating the water required 1.38 mol of propane. Determine the efficiency of the propane camp stove if the heat released from the stove was used to heat the water. 62.4 % 38.4% D162 % 61.6%

Copper has been used for thousands of years, either as a pure metal or in alloys. It is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. Determine the energy associated with each of these processes in order to recycle 1.40 mol Cu. The smelting of copper occurs by the balanced chemical equation: CuO(s) +CO(g) → Cu(s) +CO,(g) where AHtCuo is = - 155 kJ/mol. Assume the process of recycling copper is simplified to just the melting of the solid Cu starting at 25°C. The melting point of Cu is 1084.5°C with AH®fus = 13.0 kJ/mol and a molar heat capacity, CPCU = 24.5 J/mol:°C.

Calculate the work, w, done in kJ when a gas contracts from 55 L to 25 L against a constant external pressure of 1.5 atm. 1 L ∙ atm = 101 J

Find the work energy, w, gained or lost by the system when a sample of gas expands from 10 L to 30 L against a constant external pressure of 2.0 atm. [1L· atm = 101 J] -1.01 KJ -3.02 KJ -2.02 KJ 4.04 KJ

Calculate ΔHrxn for the reaction: 7 C (s) + 8 H2 (g) → C7H16 (g) The following reactions and associated ΔHrxn values are may likely be helpful to you: Reaction A: C7H16(g) + 11 O2 (g) → 7 CO2 (g) + 8 H2O (g) ΔHrxn = -4817 kJ Reaction B: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ Reaction C: 2 H2 (g) + O2 (g) → 2 H2O (g) ΔHrxn = -483.6 kJ

The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?

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.)

Energy in the amount of 5.0 J is added to 0.50 g pieces of aluminum, copper, and magnesium that are initially kept at 22 °C. The molar heat capacities of these metals are 24.3 J/(mol·°C), 24.5 J/(mol·°C), and 24.9 J/(mol·°C), respectively. Which piece of metal will have the highest temperature and what is that temperature?