The heat of combustion of liquid fuel is 2021 kJ/mol. How much of the fuel is needed to produce a heat amount of 750 kJ? The molarmass of the fuel is 60 grams per mole. Its density is 0.804 g/mL.a. 21.2 gramsO b. 162 gramsc. 27.7 gramsO d. 22.3 gramsO e. 130 grams

Answered: Image /qna-images/answer/3eeea778-b3b4-42a1-9bb0-1d0047a11891.jpg

Answered: The heat of combustion of liquid fuel…

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

#18
22. Consider the following reaction. N2 + 3 H2 -> 2 NH3 ΔH = -92 kJ/mol How many grams of nitrogen gas react if 45 kJ of energy is released? A.4140 g B.148 g C.6.85 g D.13.6 g
A 22.0 g piece of metal is heated to 100.0°C and placed in 75.0g of water at 25.0°C. if the final temperature of the metal and water is 27.8°C, what is the specific heat capacity of the metal in J/g°C? The specific heat capacity of water is 4.184 J/g°C. а. 0.038 b. 0.16 c. 0.55 d. 5.0 a
3. A certain quantity of nitrous oxide (laughing gas) expands, doing 144 J of work. At the same time, it absorbs 299 J of heat from the surroundings. Which ONE represents the change in internal energy of the nitrous oxide? A. B. C. D. E. -443 J -155 J OJ 155 J 443 J
2. A solid substance has a mass of 250 grams. It is cooled by 25.00°C and loses 4.937 kJ of heat. What is the specific heat capacity of the substance? 20 3. A 10.0 g sample of pure acetic acid, CH3CO2H, is completely burned. The heat released warms 2.0 L of water from 22.3°C to 39.6°C. I MAR a) Assuming that no heat was lost to the calorimeter, what is the molar enthalpy change of the complete combustion of acetic acid? Express your answer in kJ/mol. b) Will the bonds in the products be longer or shorter than the bonds in the reactants?
Which of the following below are endothermic process(es)? One or more processes may be chosen. Explain why. a. In the freeze-drying of coffee, ice is converted directly to gas at low temperature and pressure. b. In a fractionating column, components of crude oil vapors liquify at different levels according to their boiling points. c. In the hands of an artist, molten glass is shaped into glass ornaments of various shapes and sizes. d. When melted, the S8 ring of sulfur breaks to form long linear chains (S16, S24, etc.).
ature of a 12.58 g sample of calcium carbonate [CaCO,(s)] decreases from 382 C to 23.6 C the specific heat of calcium carbonate is 0.82 J/g-K, how many joules of heat are lost to the surroundings? Select one: O a. 151 O b. 7.5 OC.-5.0 O d. -0.82 e. -138
4. The heat capacity of copper is 0.382 J/g°.C. A 22.6 g sample of copper at 93° C is placed in 50 g of water at 23.9° C. What is the final temperature of the system?
A sample of 175°C copper is placed into a beaker with 100 grams of 25°C water. Which sample of copper will heat the water to the lowest final temperature? The specific heat of copper is 0.385 J-g-1.°C-1. The specific heat of water is 4.184 J·g-1.°C-1. A. 5.0 g Cu B. 2.0 g Cu C. 0.5 g Cu D. 1.0 g Cu
6. A metal bar with a specific heat of 0.611J/g Cthat has been heated to100.0 "C is placed into a calorimetes containing 25.0g of water at a temperature of 23.0 °C. The final temperature of the system is 32.7 "C. What is the mass of the metal?
A 50.0-g piece of metal at 80.0 °C is placed in 100 g of water at 22.0 °C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6 °C. Water has a heat capacity of 4.18 J/g°C. a. How much heat did the metal give up to the water? b. What is the specific heat capacity of the metal? c. If it is one of the substances found in Table 5.1, what is its likely identity?
Consider the following reaction: C3H8 + 5 O2 --> 3 CO2 + 4 H2O If the overall reaction has an enthalpy of reaction of -2220 kJ/mol, and water has a heat of formation of -286 kJ/mol, what mass of water is produced when 3500 kJ of energy is released? a. 0.35 g b. 28 g c. 114 g d. 881 g

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

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

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

The heat of combustion of liquid fuel is 2021 kJ/mol. How much of the fuel is needed to produce a heat amount of 750 kJ? The molar mass of the fuel is 60 grams per mole. Its density is 0.804 g/mL O a. 21.2 grams O b. 162 grams O c. 27.7 grams O d. 22.3 grams O e. 130 grams