wires heat sample Water Stirrer nud Sample buming Steel sample outside chamber In an experiment, a 0.5315 g sample of 1-naphthoic acid (Cu HaO₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.091 x 10³ g of water. During the combustion the temperature increases from 21.63 to 24.37 "C. The heat capacity of water is 4.184 J-g¹.0¹. The heat capacity of the calorimeter was determined in a previous experiment to be 983.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1-naphthoic acid based on these data. C₁ H₂O₂(0)+120₂ (9) 4H₂O()+11C0₂(g) + Energy kJ/mol Molar Heat of Combustion -

wires heat sample Water Stirrer nud Sample buming Steel sample outside chamber In an experiment, a 0.5315 g sample of 1-naphthoic acid (Cu HaO₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.091 x 10³ g of water. During the combustion the temperature increases from 21.63 to 24.37 "C. The heat capacity of water is 4.184 J-g¹.0¹. The heat capacity of the calorimeter was determined in a previous experiment to be 983.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 1-naphthoic acid based on these data. C₁ H₂O₂(0)+120₂ (9) 4H₂O()+11C0₂(g) + Energy kJ/mol Molar Heat of Combustion -

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 22.1g piece of aluminum (which has a molar capacity of 24.03 J/oC.mol) is heated to 82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is 4.18J/goC) initially at 22.3oC. The final temperature of the water is 25.8oC. Ignoring significant figures, calculate the mass of the water in the calorimeter.
A 0.4554g sample of sucrose (C12H22O11) is burned in a calorimeter which has a calorimeter constant of 333 J/℃. The calorimeter contains 500.0g of water. If the temperature of the water and calorimeter increase by 3.093℃, a) Calculate the heat given off by the burning sucrose. b) Calculate the molar heat of combustion of sucrose (that is, the heat which would be given off by the combustion of one mole of sucrose).
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.
A 1.595 g samples of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.67 degrees Celsius to 29.44 degrees Celsius. The heat capacity (calorimeter constant) of the calorimeter is 30.29 kJ/degrees Celsius, what is the heat of combustion per gram of the material?
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?
10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C
When 9.1 g of a hydrocarbon is combusted in a bomb calorimeter the temperature of the calorimeter increases from 23.8 C to 53.5 C. The calorimeter contains 731 g of water and the heat capacity of the bomb is 872 J/ C. Please calculate q rxn, in kJ, for the combustion of the hydrocarbon.
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 chemist wastes a delicious brownie by burning it in a bomb calorimeter. before burning, the brownie weighed 16.13 grams. During the combustion process in the bomb calorimeter, the heat of the calorimeter increased by 7.40 degrees celsius. The known heat capacity of the calorimeter that was used was 26.53 kJ/Celsius. What is the energy content, in kJ/g, of this brownie?
A 32.1 g piece of aluminum (which has a molar heat capacity of 24.03 J/°C·mol) is heated to 82.4°C and dropped into a calorimeter containing water (specific heat capacity of water is 4.18 J/g°C) initially at 22.3°C. The final temperature of the water is 25.8°C. Calculate the mass of water in the calorimeter.
75.0 mL of 1.80 M CuSO 4 solution is mixed with 150 mL of 1.80 M NAOH solution in a coffee cup calorimeter of negligible heat capacity. If the initial temperature of the two solutions are both 21.0 degrees C, and the final temperature of the mixed solution is 27.1, how much heat was released by the reaction? Assume density of solution d is 1.00 g/mL and that the solution has the same specific heat as water. The thermochemical equation is: CuSO4 (ag) + 2NAOH (ag) --> Cu(OH)2 (s) + Na SO4 (ag) AH xn = - 42.3 kJ/mol rxn Hint: no limiting reagent, substances are presented in correct molar ratios. O 6180 J O 9270 J O 3120 J O 5740 J O 9300 J O 1250 J O 6230 J O 3380 J
When 1.366 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?