What does a well-insulated calorimeter prevent from entering or leav- ing the system? A gases light energy solids thermal energy

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.

A 5.71 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 °C. After the salt has completely dissolved, the temperature of the solution is 28.54 °C. Was the dissolution process endothermic or exothermic?

Carbon monoxide (co) reacts with h2O to make carbon dioxide (CO2) and hydrogen gas (H2). All molecules in the balanced equation have a coefficient of 1 and the reaction is reversible. Write the equation for this reversible reaction using appropriate symbols.

A gas is compressed from an initial volume of 5.70 L to a final volume of 1.24 L by an external pressure of 1.00 atm. During the compression the gas releases 125 J of heat. What is the change in internal energy of the gas?

Please help with questions 5-12. Note: mass of HCl solution = 50.0g and mass of NaOH solution = 50.0g

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 1.19 mol Cu. The smelting of copper occurs by the balanced chemical equation:CuO(s)+CO(g)---->Cu(s)+CO2​(g)where ΔH°f,CuO 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 ΔH°fus = 13.0 kJ/mol and a molar heat capacity, cP,Cu = 24.5 J/mol·°C.   a. Enthalpy change for the reaction recovering Cu from CuO             kJ    b. Energy for recycling Cu                 kJ

Ice at 0.0 °C is placed in a Styrofoam cup containing 372. g of a soft drink at 15.4 °C. The specific heat of the drink is about the same as that of water. Some ice remains after the ice and soft drink reach an equilibrium temperature of 0.0 °C. Determine the mass of ice that has melted. Ignore the heat capacity of the cup. (Hint: It takes 334 J to melt 1 g of ice at 0.0 °C.) Be sure your answer has the correct number of significant digits. Note: Reference the Phase change properties of pure substances table for additional information. 1 6.D g x10 Ś

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 ?

A reaction where the products are higher in energy than the reactants is an example of an exothermic process endothermic process exergonic process