Many power plants produce energy by burning carbon-based fuels, which also produces carbon dioxide. Carbon dioxide is a greenhouse gas, so over-production can have negative effects on the environment. Use enthalpy of formation data to calculate the number of moles of CO₂(g) produced per megajoule of heat released from the combustion of each fuel under standard conditions (1 atm and 25 °C). coal, C(s, graphite) natural gas, CH₂(g) propane, C₂H₂(g) octane, CH₁, AH; = -250.1 kJ mol-¹ x10 TOOLS mol MJ-1 mol MJ-1 mol. MJ-1 mol MJ-1

4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6

As a system increases in volume, it absorbs 52.0 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.597 atm. The final volume of the system is 58.6 L. What was the initial volume of the system if the internal energy of the system decreased by 106.2 J? Volume =  L

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.

22. A 44.97−g sample of water at 72.2°C is added to a sample of water at 25.7°C in a constant-pressure calorimeter. If the final temperature of the combined water is 38.4°C and the heat capacity of the calorimeter is 26.3 J/°C, calculate the mass of the water originally in the calorimeter.

A gaseous fuel mixture contains 23.2% methane (CH4), 40.8% ethane (C₂H6) and the rest propane (C3H8) by volume. Part A When the fuel mixture contained in a 1.55 L tank, stored at 756 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.) Express your answer with the appropriate units. μA Value Units Review | Constants | Periodic Table ?

What is the enthalpy of reaction, ΔHrxn for the reaction of nitrogen gas with oxygen gas to produce NO2(g), based on the following information? These reactions are not at standard state or at 298 K. N2(g) + O2(g) → 2 NO(g); ΔH = 332.9 kJ2 NO2(g) → 2 NO(g) + O2(g); ΔH = 718.4 kJ Report your answer in kJ to 1 decimal place.

Please don't provide handwritten solution ..

A quantity of 100.0 mL of 1.0 M HCl and 100.0 mL of 1.0 M NaOH are mixed in a calorimeter. The initial temperatures of the HCl and NaOH solutions are the same at 20.0°C and the final temperature of the mixture is 27.0oC.  Calculate the heat of neutralization for the reaction in kJ/mole of NaOH.  Assume the density and specific heat of the solutions are the same as pure water and that no heat was lost to the surroundings.

Measurements show that the energy of a mixture of gaseous reactants decreases by 374. 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 176. 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 endothermic 0x1 x10 X Ś