When 2348 J of heat energy is added to 48.6 g of ethanol, C2H6O, the temperature increases by 19.7 ∘C. Calculate the molar heat capacity of C2H6O.

In titrating 0.20 M hydrochloric acid, HCl, with 0.20 M NaOH at 25°C, the solution at the equivalence point is Select one: a. 0.20 M NaCl b. very acidic c. slightly acidic d. 0.10 M HCl and 0.20 M NaOH e. 0.10 M NaCl

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

When 0.0901 mol of an unknown hydrocarbon is burned in a bomb calorimeter, the calorimeter increases in temperature by 2.19°C. If the heat capacity of the bomb calorimeter is 1.229 kJ/°C, what is the heat of combustion for the unknown hydrocarbon?

A piece of metal of mass 15 g at 99◦C is placed in a calorimeter containing 41.3 g of water at 19◦C. The final temperature of the mixture is 40.2◦C. What is the specific heat capacity of the metal? Assume that there is no energy lost to the surroundings. Answer in units ofJg·◦C.

When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)

The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.64g of glucose is burned in a calorimeter containing 788 g of water, and the temperature of the assembly increases from 20.10oC to 24.16oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol.

Suppose 2.32 kJ of heat is added to 25.4 g of ethanol at 18.71 °C. The specific heat capacity of ethanolis 2.46 J/g °C. What is the final temperature of the ethanol?