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

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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...

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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
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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
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50.25 g of metal that is at a temperature of 10.0 C is placed into 45.0 g H2O which is at 21.5 c, the final temperature of both metal and H2O is 30.3 C. (Given: CH2O = 4.18 J/g C) a. calculate the heat gained by the H2O. b. calculaye the specific heat of the metal c. calculate the density of the hydrogen gas at 30.0 C and 750 mm pressure. (R= 0.0821 L atm/K mol)

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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