Water is a poor heat conductor, but a pot of water can be heated more quickly than you might think. The faster than expecting heating time is probably due to what additional mechanism?
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- A high-end gas stove usually has at least one burner rated at 14 000 Btu/h. (a) If you place a 0.25-kg aluminum pot containing 2.0 liters of water at 20°C on this burner, how long will it take to bring the water to a boil, assuming all the heat from the burner goes into the pot? (b) Once boiling begins, how much time is required to boil all the water out of the pot?How long does it take a 750-WW coffeepot to bring to a boil 0.85 LL of water initially at 18 ∘C∘C? Assume that the part of the pot which is heated with the water is made of 360 gg of aluminum, and that no water boils away. Ignore the heat loss to the surrounding environment. The value of specific heat for water is 4186 J/kg⋅C∘J/kg⋅C∘ and for aluminum is 900 J/kg⋅C∘J/kg⋅C∘. Express your answer using two significant figures. In secondsAn uninsulated container holds 3.5 mol of an ideal gas at an initial temperature of 300 K. The gas is compressed by a movable piston, and 500 J of work is done on the gas while being compressed. If the final temperature of the gas is 400 K, how much heat flows in or out of the gas during this process?
- Typical freshly cut "green" firewood contains about 50% water by weight; for seasoned wood, the comparable figure is about 20%. Firewood is usually sold by volume, so compare the energy available from a given volume of green wood with that available from seasoned wood. Assume an energy content of 20 MJ/kg for perfectly dry wood, and that 2.3 MJ/kg of energy is needed to vaporize water. Also assume that the wood has essentially the same volume whether green or seasoned.In testing a new drug, you heat a 0.5-kilogram sample using a hot plate. Assume no energy is lost in the process (i.e. the process is 100% efficient). The corresponding change in temperature and energy readings observed during the heating process are graphed as shown. Watch your units!!!! 16000 14000 12000 10000 8000 Q= 72 AT 6000 4000 2000 100 150 200 250 Change in Temperature (AT) [deg F] What is the specific heat capacity of the fluid in units of joules per gram kelvin? Hint: compare the trendline equation to the thermal energy equation. * A Energy (Q) [J]You have a spherical heater, outside diameter = 3.40 cm, immersed in a container of water. In order to keep the water in the container heated to a constant temperature of 35.0°C you adjust the temperature of the spherical heater. You reach a steady-state condition when the surface temperature of the spherical heater is at 79.0°C. Assuming the electrical efficiency of the heater is 100.0%, calculate the power required by the heater (i.e., calculate q). Ignore radiation.
- An ice block of mass 1.2000000000000002 kg at an initial temperature of –11 ∘C is put into a copper pot of mass 2.5 kg containing 4.3 L of water at 21 ∘C. If you heat up the pot, what is the amount of energy (in J) you need to convert all the ice and the water into steam? (Assume that no energy is lost from the system.) You may need some or all of the following constants: The specific heat of ice is 2200 J/kg ∘C, the specific heat of copper is 386 J/kg ∘C and the specific heat of water is 4186 J/kg ∘C. The latent heat of fusion of ice is 334000 J/kg and the heat of vaporization for water is 2256000 J/kg .As ice melts in a drink, is the heat gained by the ice equal to the heat lost by the drink? If it is in an insulated cup (like styrofoam)? I tried to calculate the values and what I got for the heat lost by the drink was a much larger number than heat gained by the ice after it meltsA container holding 4.20 kg of water at 20.0°C is placed in a freezer that is kept at -20.0°C. The water freezes and comes to thermal equilibrium with the interior of the freezer. What is the minimum amount of electrical energy required by the freezer to do this if it operates between reservoirs at temperatures of 20.0°C and –-20.0°C? (Latent heat of fusion of ice = capacity of water = 4186 J/(kg K), specific heat capacity of ice = 2100 J/(kg K)). 333,700 J/ kg, specific heat kJ