Mass of can (g) Mass of can and water (g) Initial mass of food sample (g) Final mass c food sample (g) Initial temperature of water (C) Final temperature of water ("C) Mass of water (g) Temperature change of water ("C) (Do not include a negative sign) Heat gained by water (cal) (Do not include a negative sign) Heat gained by water (kcal) (Do not include a negative sign) Heat lost by food (cal) (Do not include a negative sign) Heat lost by food (kcal) (Do not include a negative sign) Mass of food burned (g) Calories per gram of food (kcal/g) Quantity 12.678 126.225 1.879 0.450 23.2 25.0

Mass of can (g) Mass of can and water (g) Initial mass of food sample (g) Final mass c food sample (g) Initial temperature of water (C) Final temperature of water ("C) Mass of water (g) Temperature change of water ("C) (Do not include a negative sign) Heat gained by water (cal) (Do not include a negative sign) Heat gained by water (kcal) (Do not include a negative sign) Heat lost by food (cal) (Do not include a negative sign) Heat lost by food (kcal) (Do not include a negative sign) Mass of food burned (g) Calories per gram of food (kcal/g) Quantity 12.678 126.225 1.879 0.450 23.2 25.0

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

Please help me
A) 2100 calcal to kcalkcal B) 425 JJ to cal C) 2.4 kJkJ to cal
aluminum metal has a specific heat of 0.901 j/g*c. How much heat is transferred to a 6.75 g peice of aluminum initially at room temperature, 20.0*c when it is placed into boiling water? The temperature of boiling water is 100*C.
A metal is thought to be copper or gold. When 18 g of the metal absorbs 58 cal, its temperature rises by 35 ̊C. a) What is the specific heat, in cal/g ̊C, of the metal? b) Would you identify the metal as copper or gold?
Gasoline is composed of a variety of different liquid hydrocarbons, which do not separate as time passes. Gasoline is an example of a: A) heterogeneous mixture B) Chemical compound C) Chemical element D) Solution
Name (please print): Heat Capacity of an Unknown Metal Post Lab Questions 1.) When determining the heat capacity of the unknown metal we assumed the heat capacity of the water has a value of 4.186J/g®C. Is there an error(s) in making this error? Explain The possibility of error in the experiment can be loss of heat, the thermometer not being precise enough to give accurate values, and the capacity of the thermometer is being ignored 2.) What is the heat energy needed to raise the temperature of 6.63moles of ethanol CH;CH;OH from a temperature of 2.33°C to 17,5°C. [CH;CH;OH=46.07g/mol) [Ccusch2ow-2,46J/g°C] 3.) What is the identity of an unknown metal that absorbs 0.589KJ of heat energy where the metal is heated from 33.6°C to 241.6°C. The mass of the metal is 13.48g. [Cr= 0.160 J/g°C] [Cs»= 0.210 J/g°C] [Cc. = 0.385 J/g°C][Cz» = 0_390 J/g*C] 4.) How much encrgy is liberated when 600.2g of O, is reacted with propane in a combustion tank. Assume the following: C,Hg) + 50;(g) – 3C0;(g)+…
Each blank only has one correct answer: Answer choices for A: a. 0 b. 1 c. 2 d.3 e.4 Answer choices for D: a. 0 b. 1 c. 2 d.3 e.4
Show how to determine and then calculate the final temperature of a 195 g copper pan when 5925 calories of energy are added to the copper pan that is initially at 24.5 degrees celsius. (the specific heat of copper is 0.0923 cal/g degrees celsius)
question is in the photo
Aluminum has a specific heat of 0.902 J/g⋅°C. How many joules of heat are required to change the temperature of 8.50 grams of aluminum from 25.0°C to 93.4°C? a) 7.67 J b) 71.7 J c) 192 J d) 483 J e) 524 J
The specific heat of aluminum is 0.900 j/g*C, how many joules of energy are required to raise the temperature of 20.0 g of Al from 10.0 C to 15.0 C ?
Identity of metal Mass of metal, (g) Copper 31.715 Trial 1 Mass of Styrofoam® cup and water, (g) 110.850 Mass of Styrofoam® cup, (g) 9.925 Trial 2 88.845 10.385 g Mass of water, (g) 100.925 78.46 Initial temperature of metal (Temperature of the boiling water) 90°C 98.5°C Initial temperature of water in cup, 22.5°C 22.5°C Final temperature of water and metal 25°C Specific heat of metal, (cal/g° C) Average specific heat of metal, (cal/g 33% 25°C 2.95% C) Calculations: ATwater Tf- Ti water °C ATmetal Tf-Ti metal ос = Qwater (1.00 cal/g°C) x ( _g H2O) x (°C) = cal Qmetal = - Qwater Cmatel Ometal/mmetal X ATmetal=- cal/[C g)x( °C)] = _cal/g°C