Part A A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 101 g of solution. The reaction caused the temperature of the solution to rise from 21.0 24.7°C. What is the molar reaction enthalpy? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water Use data from the "Formula Sheets" or the "Tables posted on Canvas (see "Module 0: Important Files") for any additional information. Enter your answer with three significant figures in the given unit. The margin of error is 2%. ▸ View Available Hint(s) ΕΠΙ ΑΣΦ ?

Suppose 200.0 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH, both initially at 25.0°C, are mixed in a thermos flask. When the reaction is complete, the temperature is 28.4°C. Assuming that the solutions have the same heat capacity as pure water, compute the heat released (in kJ).

A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods.   In an experiment, a 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C.   The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C.   Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data.   Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol).   C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy

Suppose 300 mL of 2.00 M HCl and 300 mL of 2.00 M NaOH, both initially at 23.0 celsius, are mixed in a thermos flask. When the reaction is complete, the temperature is 36.6 celsius. Assuming that the solutions have the same heat capacity as pure water, compute the heat released in kJ