When 1177 J1177 J of heat energy is added to 39.1 g39.1 g of hexane, C6H14,C6H14, the temperature increases by 13.3 ∘C.13.3 ∘C. Calculate the molar heat capacity of C6H14.

Part B 2.0000 g of the unknown compound is burned in a bomb calorimeter. During the combustion, the temperature of the calorimeter increases from 23.125°C to 28.997 °C. During calibration, the heat capacity of the calorimeter was found to be 9.9897kJ °C-1. In the previous experiment, the molar mass of the substance was found to be 148.16 gmol-1. What is AcombU for the unknown compound? να ΑΣφ ? kJ mol1 Submit Request Answer

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.

A sample of iron, which has a specific heat capacity of 0.449 J.g¹.°C¹, is put into a calorimeter (see sketch at right) that contains 100.0 g of water. The iron sample starts off at 98.2 °C and the temperature of the water starts off at 23.0 °C. When the temperature of the water stops changing it's 27.4 °C. The pressure remains constant at 1 atm. Calculate the mass of the iron sample. Be sure your answer is rounded to 2 significant digits. 1 g x10 X 5 thermometer. insulated container water sample a calorimeter

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 0.3215 g sample of phenanthrene (C14H10) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.162×10 g of water. During the combustion the temperature increases from 25.15 to 27.48 °C. The heat capacity of water is 4.184 J glc-!. The heat capacity of the calorimeter was determined in a previous experiment to be 769.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of phenanthrene based on these data. C14H10(s) + (33/2) O,(g) – → 5 H,O(1) + 14 CO2(g) + Energy Molar Heat of Combustion = kJ/mol

Hw.77.

A researcher studying the nutritional value of a new candy places a 4.90 g4.90 g sample of the candy inside a bomb calorimeter and combusts it in excess oxygen. The observed temperature increase is 2.44 ∘C.2.44 ∘C. If the heat capacity of the calorimeter is 42.50 kJ⋅K−1,42.50 kJ⋅K−1, how many nutritional Calories are there per gram of the candy?

When 1786 J1786 J of heat energy is added to 45.9 g45.9 g of hexane, C6H14,C6H14, the temperature increases by 17.2 ∘C.17.2 ∘C. Calculate the molar heat capacity of C6H14.C6H14. ?P=CP=   J/(mol⋅∘C)

A 3.450 g of propane (molar mass = 44.11 g/mol) was placed in a bomb calorimeter with excess oxygen and ignited. The initial temperature of the calorimeter was 24.000 degrees celsius and its total heat capacity was 76.65 kJ * C^-1. The reaction raised the temperature of the calorimeter to 28.965 degrees celsius.  a. What is the heat exchangged by the reaction in kilojoules, qrxn?  b. Calculate the deltaE rxn for the combustion of propane in kilojoules per mole c. Work in this reaction is done on the system, done on the surroundings, or equal to zero? Why?

A 25.0 mL portion of dilute HCl (aq) is combined with a 25.0 mL portion of dilute NaOH in a coffee-cup calorimeter. Both solutions are initially at a temperature of 23.3 ºC. The reaction produces enough heat to raise the final temperature of the 50.0 mL of liquid in the calorimeter to 25.3 ºC . What is qrxn in J? Assume the density of the reaction mixture is 1.0 g/mL and the specific heat of the solution is 4.184 J/g· ºC