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.

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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A coffee-cup calorimeter is filled with 150.0 mL of water at 22.1 °C. A piece of metal at 121.4 °C with a mass of 16.5 g is added. The final temperature of the water and metal in the calorimeter is 24.5 °C. The density of liquid water is 1.00 g/mL, and its specific heat capacity is 4.18 J/(g·°C). Determine the specific heat capacity of the metal. a) 1.40 J/g∙oC b) 0.40 J/g∙oC c) 4.18 J/g∙oC d) 0.94 J/g∙oC
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 67.75 gram sample of iron (with a heat capacity of 0.450 J/g °C) is heated to 100.0 °C. It is then transferred to a coffee cup calorimeter containing 42.29 g of water (specific heat of 4.184 J/ g °C) initially at 20.63 °C. If the final temperature of the system is 23.59, how much heat was absorbed by the calorimeter? Record your answer as a whole number (assume the sign is positive). Submit Question div Mach k Air 20 F1 F2 F3 F4 F7 %24 %23
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.
R Please don't provide the handwriting solution
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?