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In a coffee-cup calorimeter, 110.0 mL of 1.3 M NaOH and 110.0 mL of 1.3 M HCl are mixed. Both solutions were originally at 25.0°C. After the reaction, the final temperature is 33.7°C. Assuming that all the solutions have a density of 1.0 g/cm^3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbon dioxide, and the energy of sunlight to create glucose. A 0.1959-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/°C. The temperature of the calorimeter increases by 3.1°C. Calculate the energy of combustion of quinone per gram and per mole. Consider the dissolution of CaCl2: CaCl2(s) ----> Ca^2+(aq) + Cl^-(aq) ΔH = -81.5 kJ An 11.2-g sample of CaCl2 is dissolved in 123 g water, with both substances at 25.7°C. Calculate the final temperature of the solution assuming no heat loss to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/°C·g.

          In a coffee-cup calorimeter, 110.0 mL of 1.3 M NaOH and 110.0 mL of 1.3 M HCl are mixed. Both solutions were originally at 25.0°C. After the reaction, the final temperature is 33.7°C. Assuming that all the solutions have a density of 1.0 g/cm^3 and a specific heat capacity of 4.18 J/°C·g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbon dioxide, and the energy of sunlight to create glucose. A 0.1959-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/°C. The temperature of the calorimeter increases by 3.1°C. Calculate the energy of combustion of quinone per gram and per mole.

Consider the dissolution of CaCl2:
CaCl2(s) ----> Ca^2+(aq) + Cl^-(aq)  ΔH = -81.5 kJ

An 11.2-g sample of CaCl2 is dissolved in 123 g water, with both substances at 25.7°C. Calculate the final temperature of the solution assuming no heat loss to the surroundings and assuming the solution has a specific heat capacity of 4.18 J/°C·g.

Added by Gabriela P.

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