1. A 5.000 g sample of methanol, CH,OH, was combusted in the presence of excess oxygen in a bomb calorimeter containing 4000 g of water. The temperature of the water increased from 24.000 °C to 29.765 °C. The heat capacity of the calorimeter was 2.657 kJ C. The specific heat of water is 4.184 J/g°C. Calculate AE for the reaction in kJ/mol.

15.0 mL of a strong base is added to 15.0 mL of a strong acid in a coffee cup calorimeter. The temperature of the calorimeter contents rises from 22.5 °C to 24.5 °C.  Assume that: concentration of base = 0.500 M concentration of acid = 0.500 M the specific heat of the solution is 4.184 J/g°C the density of the solution is 1.00 g/mL the coffee cup does not absorb or release energy itself Calculate the ΔH for this neutralization reaction in kJ per mole of base.   Answer Options: A. –0.299 kJ/mol B. –33.5 kJ/mol C. –16.7 kJ/mol D. –0.502 kJ/mol

A 93.82 g bar of iron was heated to 98.4 °C and then dropped into 38.1 mL of water at 15.3 °C.  The temperature of the water increased to a maximum of 32.7 °C.  Calculate the specific heat capacity of iron.  Assume that the density of water is 1.00 g/mL. heat capacity (J/g°C)

In a coffee-cup calorimeter, 130.0 mL of 1.1 M  NaOH and 130.0 mL of 1.1 M  HCl are mixed. Both solutions were originally at 20.7°C. After the reaction, the final temperature is 28.1°C. Assuming that all the solutions have a density of 1.0  g/cm3 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.

In a coffee-cup calorimeter, 120.0 mL of 1.0 M NaOH and 120.0 mL of 1.0 M  HCl are mixed. Both solutions were originally at 26.1°C. After the reaction, the final temperature is 32.8°C. Assuming that all the solutions have a density of 1.0 g/cm3 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.

In a coffee-cup calorimeter, 110.0 mL of 1.4 M NaOH and 110.0 mL of 1.4 M HCl are mixed. Both solutions were originally at 24.0°C. After the reaction, 3 the final temperature is 33.4°C. Assuming that all the solutions have a density of 1.0 g/ cm° 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. ΔΗ - kJ/mol

A hot metal weighing 65.0 g was heated to 125 oC and dropped into 75.0 g of water kept at a room temperature of 20.6 oC in a calorimeter. Within a couple of minutes, water’s temperature increased to 26.8 oC and stayed constant at that temperature. If the heat capacity of calorimeter constant is 11.5 J/oC, find the specific heat capacity of the metal.

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

5. A 1.500-g sample of a hydrocarbon is placed in a bomb calorimeter and undergoes combustion. The temperature of the calorimeter rises from 20.00°C to 23.55°C. If the calorimeter has a heat capacity of 40.3 J/°C, what is the heat of combustion (qv) for this hydrocarbon in kJ/g? 6. The heat of sublimation for iodine is 62.4 kJ/mol, at 25°C and 1.00 atm. What is AE for the sublimation of iodine (shown below) under these conditions? 2 (s) F 2 (g) volsd 7. A bomb calorimeter with heat capacity of 1.500x103 J/°C was used to study combustion of terbium (Tb) in excess oxygen: 4 Tb (s) + 3 O2 (g) →2 Tb2O3 (s) When 1.000-g of terbium was burned, a temperature increase of 3.908°C was observed. What is the AE for the reaction, in kJ/mol of Tb2O3?

In a coffee-cup calorimeter, 100.0 mL of 1.1 M    NaOH and 100.0 mL of 1.1 M   HCI are mixed. Both solutions were originally at 22.8°C. After the reaction, the final temperature is 30.2°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 HCI  by NaOH . Assume that no heat is lost to the surroundings or to the calorimeter. ΔH = ---------  kJ/mol