QUESTION 12Complete combustion of 2.3 g liquid ethanol, C2H5OH in a calorimeter raised thetemperature of 3000 mL of water by 10°C. The specific heat capacity of water is4.18 Jg-1°C-1, and the density of water is 1.0 g mL-1.a) Calculate the heat of combustion, AH of C2HSOH in kJ mol-'.b) Write the thermochemical equation for the combustion of liquid C2HSOH.

Answered: Image /qna-images/answer/cffe888c-9f62-4e32-a4db-a28e7026c906.jpg

QUESTION 12 Complete combustion of 2.3 g liquid ethanol, C2H5OH in a calorimeter raised the temperature of 3000 mL of water by 10°C. The specific heat capacity of water is 4.18 Jg°C-, and the density of water is 1.0 g mL-1. a) Calculate the heat of combustion, AH of C2HSOH in kJ mol. b) Write the thermochemical equation for the combustion of liquid C2HSOH.

QUESTION 12 Complete combustion of 2.3 g liquid ethanol, C2H5OH in a calorimeter raised the temperature of 3000 mL of water by 10°C. The specific heat capacity of water is 4.18 Jg°C-, and the density of water is 1.0 g mL-1. a) Calculate the heat of combustion, AH of C2HSOH in kJ mol. b) Write the thermochemical equation for the combustion of liquid C2HSOH.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 16QAP: Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an...

See similar textbooks

Similar questions

Question 2:The standard enthalpies of formation, at 25.00 oC, of methane (CH4(g)), water (H2O(l)), and carbon dioxide (CO2(g)) are -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol respectively. Calculate the heat released (in kJ) during combustion of 18.84 L of methane under a constant pressure of 1,000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
The enthalpy of combustion of isooctane (C8H18(l)) is -5461 kJ/mol. From data found in appendix G, calculate the enthalpy of formation of C8H18(l): C8H18(l) + 12.5 O2(g) → 8 CO2(g) + 9 H2O(l) ∆Hrxn = -5461 kJ ∆Hf = ___ kJ/mol Correct answer is not 259.2
The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.09g of glucose is burned in a calorimeter containing 826 g of water, and the temperature of the assembly increases from 20.10oC to 24.70oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol. (Final answer: TWO decimal places)
Please answer the following question: The combustion of isoctane reaction produces -5099.5 kJ of heat per mole of C8H18(g) consumed, under standard conditons. The enthalpy of formation (DHf) for CO2(g) and H2O(g) are -393.5 kJ/mol and -241.8 kJ/mol, repspectively. Find the standard enthalpy of formation (DHf) of this isomer of C8H18(g)? (Show work) C8H18(g) + O2(g) -> 8CO2(g) + 9H2O(g) DHrxn = -5099.5 kJ
an important flavor component of vanilla extract is vanillin C8H8O3 molar mass = 152.15 g/mol when vanillin burns in a bomb calorimeter with a heat capacity of 8.60 kJ/°C the temp increases from 25.97°C to 31.18°C. if the heat of combustion of vanillin is -3760 kJ/mol what mass of vanillin (in g) was combusted? answer to two decimal places
Gasoline contains a mixture of alkanes, some of which are octanes, C8H18 (l). The heat of the reaction is -5471 kJ/mol of energy. The per mole is the coefficient in front of the compound in the equation. If your tank holds 10 gallons of gasoline, how much energy of combustion is available, assuming the gasoline was pure octane? Density octane = 0.7025 g/mL and 1 gallon = 3.785 L
If the enthalpy of C12H22O11 combustion is said to be -5.65 x 103 kJ/mol, calculate the mass of C12H22O11 needed to be burned to produce 2.6 kJ of heat. (MM of sucrose: 342.3)
For a particular isomer of C8H18, the combustion reaction produces 5108.7 kJ of heat per mole of C8H18(g) consumed, under standard conditions. C8H18(g) + 25/2O2(g) yields to 8CO2(g) + 9H2O(g) Delta H= -5108.7 kJ/mol What is the standard enthalpy of formation of this isomer of C8H18(g)? (Include correct number of significant figures).
Give handwritten answer A coffee cup calorimeter is prepared, containing 100.000 g of water (specific heat capacity = 4.184 J/g K) at initial temperature 80.000 C. A salt weighing 7.308 g is quickly added. The salt has a molar mass of 178.051 g/mol. The final temperature of the solution is 51.028 C. Assume no heat loss to the surroundings. Assume the specific heat capacity of the solution is equal to that of pure water, and that the mass of the solution is equal to the mass of the solid plus the mass of water in the calorimeter. What is the molar heat of solution for the salt, in kJ/mol?
Question: I)Using the result of your calculation in (b), calculate the enthalpy of hydrogenation of butadiene, assuming the formula to be CH' = CHCH = CH2ii The experimental value for this enthalpy change is -239KJ/mol. Suggest an explanation for the difference.
How many Joules of energy are required to raise 2.5kg of water from 18.5 to 55.0 ? (specific heat of water is 4.184J/g C) in correct sig fig
Students were asked to determine the heat of reaction forthe neutralization of a newly synthesized monoprotic acid HX and NaOH. Theyfirst calibrated the styro ball calorimeter using the reaction of 15.0 mL of 0.100 MHCl and 20.0 mL of 0.0500 M KOH. This recorded a change in temperature from26.5 °C to 31.8 °C. Afterwards, they determined the heat of reaction for a mixtureof 5.00 mL, 1.00 M NaOH and 10.0 mL, 1.00 M HX. This showed an increase intemperature of 3.6 °C.i. What is the heat capacity of the calorimeter in J/℃ (∆? =-55.85??????????????kJ/mol)?ii. Write the balanced chemical and net ionic equations for the reaction of NaOHand HX .iii. What is the experimental enthalpy (in kJ/mol) for the neutralization reactionbetween HX and NaOH ?iv. Is the reaction between NaOH and HX endothermic or exothermic ?