Part A When 1.547 g of liquid hexane (C6 H14) undergoes combustion in a bomb calorimeter, the temperature rises from 26.16 C to 38.45 °C. Find AErxn for the reaction in kJ/mol hexane. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 5.79 kJ/ C. Express your answer using three significant figures.

Calculate the energy required to heat 0.40 kg of ammonia from 56.1 °C to 65.4 °C. Assume the specific heat capacity of 1 ammonia under these conditions is 4.70 J·g¯¹·K¯¹ Be sure your answer has the correct number of significant digits.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.A student heats 69.43 grams of nickel to 97.93 °C and then drops it into a cup containing 75.96 grams of water at 20.90 °C. She measures the final temperature to be 27.45 °C.The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.71 J/°C.Assuming that no heat is lost to the surroundings calculate the specific heat of nickel.Specific Heat (Ni) =  J/g°C.

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction. A student heats 65.54 grams of copper to 98.08 °C and then drops it into a cup containing 78.67 grams of water at 23.78 °C. She measures the final temperature to be 29.26 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.57 J/°C. Assuming that no heat is lost to the surroundings calculate the specific heat of copper. Specific Heat (Cu) = J/g°C.

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You burn a 13.65 g sample of an unknown chemical in a bomb calorimeter. The unknown chemical has a molar mass of 55.29 g/mol. After burning the chemical, the 152 ml of water in the bomb calorimeter increased in temperature from 25.3°C to 33.5°C. What is the molar enthalpy of combustion for this chemical? Use 4.183 J/g°C as your specific heat capacity of water.

A chemist carefully measures the amount of heat needed to raise the temperature of a 533.0 mg sample of CH,N from 53.8 °C to 68.3 °C. The experiment shows that 16.5 J of heat are needed. What can the chemist report for the molar heat capacity of CH,N? Round your answer to 3 significant digits. -1 - 1 J•mol • K x10

A chemist carefully measures the amount of heat needed to raise the temperature of a 1.54kg sample of C4H8O from 2.1°C to 19.3°C. The experiment shows that 4.33 x 10^4J of heat are needed. What can the chemist report for the molar heat capacity ofC4H8O? Round your answer to 3 significant digits.

Consider the thermochemical equation for the combustion of acetone (C3H₂O), the main ingredient in nail polish remover: C3H6O (1) + 4 O₂ (g) → 3 CO₂ (g) + 3 H₂O (g) ΔΗ° rxn = 1790 kJ If a bottle of nail polish remover contains 222 mL of acetone, what is the magnitude (the value) of heat released by the complete combustion of the acetone in the bottle? The density of acetone is 0.788 g/mL. The molar mass of acetone is 58.08 g/mol. The units are kJ. Do not include units in your answer.

Acetylene, C 2 H 2 , is used in welding torches. It releases a lot of energy when burned in oxygen. The combustion of one gram of acetylene releases 48.2 kJ. A 0.750-g sample of acetylene is burned in a bomb calorimeter ( heat capacity = 1.117 kJ / °C ) that contains 800.0 g of water. The final temperature of the bomb and water after combusion is 35.2°C. What is the initial temperature of the bomb and water?