9. Portable butane stoves are often used during camping. Consider using a butane stove to boil some water, 282 kJ of energy was used. This process usually has an efficiency of 92%. a) How much water (in mL) can be boiled from its initial temperature of 15°C to the boiling point of 100°C? Given the specific heat capacity of water is 4.18x10 J/kg°C. b) The heating process takes 11 minutes and the unit cost to use butane is $0.32/kW h. Determine the cost to boil the water.

9. Portable butane stoves are often used during camping. Consider using a butane stove to boil some water, 282 kJ of energy was used. This process usually has an efficiency of 92%. a) How much water (in mL) can be boiled from its initial temperature of 15°C to the boiling point of 100°C? Given the specific heat capacity of water is 4.18x10 J/kg°C. b) The heating process takes 11 minutes and the unit cost to use butane is $0.32/kW h. Determine the cost to boil the water.

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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2. A 32.5g cube of aluminum initially at 45.8°C is submerged into 105.3 g of water at 15.4°C. The final temperature is 17.3°C. What is the heat capacity of aluminum? Swater = 4.184 J/g°C.
Calculate the heat of reaction (in J)
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)
A material has a specific heat of 0.625 J/g°C. A 75.6 g sample of this material is heated and them placed in 35.2 g of water at 21.4 °C. The temperature of the water rises to 32.7 °C. What was the initial temperature of the material?
A 322 gram sample of metal at 78.4°C with a specific heat of 0.138 J/g°C is added to 264 grams of water at 24.2°C. Calculate the final temperature reached the metal-water mixture.
The density of aluminum is 2.7 g/cm3 and its specific heat is 0.9 J/g.0. A piece of 9.7 cm3 aluminum with an initial temperature of 125 0C is put in 120 g of water in an insulating container with a temperature of 18 0C. What will be the final temperature of the aluminum-water mixture? (Specific Heat of Water: 4.186 J/g.0C)
4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).
A sample of aluminum, initially at 5.0 °C, was placed in 18.0 g of water, initially at 25.0 °C. The final temperature of the water and the metal was 21.0 °C. The specific heat of water is 4.184 J g-1 °c-1 and aluminum is 0.940 J g-1 °C-1. Ignore the heat capacity of the container. What is the mass (in g) of the aluminum?
A block of iron weighing 3.50 kg at a temperature of 107.0 °C was inserted into a container containing 1.00 liter of water at a temperature of 30.0 °C isolated from the environment. What is the final temperature (in °C) of the water and the iron at the end of the process? (The specific heat of solid iron is 0.450 J /g and the specific heat of water is 4.184 J/ g°C ) Density of water = 1.0 g/mL.
A piece of metal with a specific heat of 1.153 J/gºC is heated to 124.6ºC and then placed in 120.382 g of water which is at a temperature of 2.1 ºC. After a minute, the temperature of the water has stopped changing and is now 45.5ºC. Assuming that there are no heat losses to the container or surroundings, what is the mass of the piece of metal in grams? Assume that water has a specific heat of 4.184 J/gºC. Enter your answer with at least 3 sig figs.