Imagine that a hypothetical life form is discovered on our moon and transported to Earth. On a hot day, this life form begins to sweat, and it is determined that the heat of vaporization of its sweat is 259 cal/g. The scientist observing the extraterrestrial life form also begins to sweat. The heat of vaporization of the scientist's sweat is 580 cal/g at the skin's surface. If both the extraterrestrial life form and the scientist lose 493 g of sweat over the course of one hour, calculate the heat lost by each body from the vaporization of sweat. extraterrestrial: cal human scientist: cal

Imagine that a hypothetical life form is discovered on our moon and transported to Earth. On a hot day, this life form begins to sweat, and it is determined that the heat of vaporization of its sweat is 259 cal/g. The scientist observing the extraterrestrial life form also begins to sweat. The heat of vaporization of the scientist's sweat is 580 cal/g at the skin's surface. If both the extraterrestrial life form and the scientist lose 493 g of sweat over the course of one hour, calculate the heat lost by each body from the vaporization of sweat. extraterrestrial: cal human scientist: cal

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

You would like to determine how many calories are in 10 grams of chicken that is served in the LaGCC cafeteria. Using your understanding of a bomb calorimeter (Figure 5.18 in your textbook) Devise a scheme to find how many calories are in the meat and Assuming the specific heat of chicken is 3.68 J/g⁰C and the change in temperature was 1.90⁰C, how many calories are in 10 grams of chicken? For the following hypothetical reactions: 2A + 3B → C + D ∆H = -46 KJ E + A → C ∆H = 50 KJ A + 0.5D → B ∆H = 23 KJ
The chemical energy in food is calculated by determining the heat transferred to a small body of water when that piece of food is combusted. Calculate the nutritional calories in a potato chip that raises the temperature of 62.658 g of water by 9.95°C.
You are given 50g of an unknown metal. You apply 6000J of energy to the metal, raising its temperature from 25°C to 955°C. What is the specific heat of the metal? What is the identity of the metal? Metal Magnesium Aluminum Potassium Calcium Specific Heat (J/g°C) 1.02 0.90 J/g°C 0.75 0.65 Metal Silver Tin Lead Gold Specific Heat (J/g°C) 0.24 0.21 0.16 0.129
When a water heater containing 118.9 liters of water is turned off, the temperature of the water drops from 75.0 °C to 22.5 °C. How much heat (in KJ) is lost to the environment? (assume that the density of the water is 1.00 g/ml).
13.0 g of cream at 22.4 °C are added to an insulated cup containing 150.0 g of coffee at 81.3 °C. Calculate the equilibrium temperature of the coffee. You may assume no heat is lost to the cup or surroundings, and that any physical properties of cream and coffee you need are the same as those of water. Be sure your answer has 3 significant digits. °C Xx10 X
Jazmin and Ty did a chemistry experiment in which they dissolved the ionic compound lithium chloride (LiCl) in water. They observed that after mixing 3.0 g of the ionic compound into 20 mL of water, the temperature dropped from 22 °C to 15 °C. Based on these experimental results, it is likely that all of the following would result in a greater temperature decrease except:
When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)
8
A student disolves 12.0 g of lithium chloride (LiCl)in 300. g of water in a well-insulated open cup. She then observes the temperature of the water rise from 20.0 °C to 27.5 °C over the course of 6.7 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: LiCI(s) - Li (aq) + Cl (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ Calculate…
If an athlete expends about 7.10 x 10² Cal/hr then how many minutes would the athlete need to run to "burn off" the Calories consumed from eating a quarter-pound cheeseburger, French fries, and a chocolate shake that contains a total of 120. g carbohydrates, 49 g of fat, and 45 g of protein. Fat Carbohydrates Proteins Calories per gram 9.0 4.0 4.0 6713100 M
A student dissolves 14.6 g of lithium chloride (LiCI)in 250. g of water in a well-insulated open cup. He then observes the temperature of the water rise from 21.0 °C to 33.5 °C over the course of 6.3 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: LiCI(s) Li (aq) + Cl (aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ Calculate the…
If you combine 360.0 mL of water at 25.00 °C and 130.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water. Tinal