Use constant-volume calorimetry to determine energy change.A 0.376-g sample of decanoic acid (C10H2002) is burned in a bomb calorimeter and the temperature increases from 24.90 °C to 27.40 °C. Thecalorimeter contains 1.05x103 g of water and the bomb has a heat capacity of 793 J/°C. Based on this experiment, calculate AE for the combustionreaction per mole of decanoic acid burned (kJ/mol).C10H2002(s) + 14 O2(g) →10 CO2(g) + 10 H2O(1)ΔΕ=kJ/molCheck & Submit AnswerShow Approach

Given, The combustion reaction : C10H20O2(s) + 14O2(g) → 10 CO2(g) + 10 H2O(I) mass of decanoic…

Use constant-volume calorimetry to determine energy change. A 0.376-g sample of decanoic acid (C10H2002) is burned in a bomb calorimeter and the temperature increases from 24.90 °C to 27.40 °C. The calorimeter contains 1.05×10 g of water and the bomb has a heat capacity of 793 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of decanoic acid burned (kJ/mol). C10H2002(s) + 14 O2(g) →10 CO2(g) + 10 H20(1) ΔΕ kJ/mol Check & Submit Answer Show Approach

Use constant-volume calorimetry to determine energy change. A 0.376-g sample of decanoic acid (C10H2002) is burned in a bomb calorimeter and the temperature increases from 24.90 °C to 27.40 °C. The calorimeter contains 1.05×10 g of water and the bomb has a heat capacity of 793 J/°C. Based on this experiment, calculate AE for the combustion reaction per mole of decanoic acid burned (kJ/mol). C10H2002(s) + 14 O2(g) →10 CO2(g) + 10 H20(1) ΔΕ kJ/mol Check & Submit Answer Show Approach

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

100.0 mL of cold water at 20.5 oC was poured into a styrofoam coffee cup calorimeter. After adding 100.0 mL of hot water at 30.5 oC and mixing it thoroughly, the temperature of the mixture was found to 24.7 oC. Find the heat capacity of the calorimeter. [Specific heat capacity of water is 4.184 J/goC. Assume density of water is 1.0 g/mL at both temperatures.]
The combustion of 0.1587 g benzoic acid increases the temperature of a bomb calorimeter by 2.57°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2140-g sample of vanillin (CHO3) is then burned in the same calorimeter, and the temperature increases by 3.25°C. What is the energy of combustion per gram of vanillin? Energy= kJ/g %3D Per mole of vanillin? Energy = kJ/mol %3D
A 6.78 g sample of methanol was combusted in a bomb calorimeter. The temperature of the calorimeter increased by 12.7 °C. If the molar mass of methanol is 32.04 g/mol, and the heat capacity of the calorimeter is 5,104 J/°C, what is the molar AE for this reaction, in kJ/mol? Do not report units in your answer. Report your answer to one decimal place and include the correct sign.
When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?
The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid.In a particular bomb calorimeter (initially at room temperature), the combustion of 0.2745 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.85 °C.When a 0.2999-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.59 °C.What is the energy of combustion per unit mass of the unknown substance?
6, A 0.213 g sample of an organic compound with a molar mass of 386.0 g/mol was burned in the bomb calorimeter with a heat capacity of 2.54 kJ/K. The temperature in the calorimeter increased by 4.12 K. Calculate the energy of combustion of the compound in kJ/mol. A, –1.896 x103 B, –4.90 x102 C, 0.00937 D, –1.90 x104 E, -531
A 3.000 g sample of food was then burned in a calorimeter to determine its Calories per gram content. 50mL of water were used to determine ΔT of the reaction. Initial temperature of the water at the start of the combustion reaction was 20oC, final temperature was 99oC. Calorimeter constant for this calorimeter is 10.0J/oC. How much heat has been absorbed by the water sample?
An electrical heater adds 25.3 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter rises by 4.55 °C. When 1.75 g of methanol is burned in the same calorimeter, the temperature increases by 7.14 °C. Calculate the molar energy of combustion of methanol. kJ/mol
The combustion of 0.1566 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2195-g sample of vanillin (Cg H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.21°C. What is the energy of combustion per gram of vanillin? Energy = kJ/g Per mole of vanillin? Energy = kJ/mol