A piece of aluminum foil used to wrap a potato for baking in a hot oven can usually be handled safely within a few seconds after the potato is removed from the oven. The same is not true of the potato, however! Give two reasons for this difference.
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A piece of aluminum foil used to wrap a potato for baking in
a hot oven can usually be handled safely within a few seconds after the
potato is removed from the oven. The same is not true of the potato,
however! Give two reasons for this difference.
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- #5Q:33)Two water bottles X and Y have the same mass (m) and very similar size and shape but are made from different materials (Mx and My respectively) at room temperature. The same amount of boiling water is put into X and Y, and then both bottles are closed with screw caps. After 5 minutes, the temperature of water in bottle X is higher than the water in bottle Y. We may then conclude that (with an explanation): (a) Mx has higher specific heat and the water in X has lower internal energy. (b) Mx has lower specific heat and the water in Y has higher internal energy. (c) My has lower specific heat but the water in X and Y have the same internal energy. (d) My has higher specific heat but the water in X has higher internal energy. (e) My and My have the same specific heat and the water in X and Y have the same internal energy.
- How much heat energy must be removed from 0.10 kg of oxygen with a temperature of 22 °C in order for the oxygen to liquefy at -183 °C? (Co = 913 J/kg°C, Ly = 2.13 x 105 J/kg and oxygen liquefies as -183 °C) O 5 x 10^4 J O 9 x 10^4 J O 1 x 10^4 J O 4 x 10^4JA pot on the stove contains 500 g of water at 20°C. An unknown mass of ice that is originally at −10°C is placed in an identical pot on the stove. Heat is then added to the two samples of water at precisely the same constant rate. Assume that this heat is transferred immediately to the ice or water (in other words, neglect the increase in temperature for the pot). We will also neglect evaporation. The ice melts and becomes water, and you observe that both samples of water reach 60.0°C at the same time. Solve for the mass of the ice that was originally in the second pot. The specific heat of liquid water is 4186 J/(kg °C), and of solid water is 2060 J/(kg °C). The latent heat of fusion of water is 3.35 105 J/kg.Two water bottles A and B have the same mass (m) and very similar size and shape but are made from different materials (MA and MB respectively) at room temperature. The same amount of boiling water is put into A and B, and then both bottles are closed with screw caps. After 5 minutes, the temperature of water in bottle A is higher than the water in bottle B. We may then conclude that (with your explanation):(a) MA has higher specific heat and the water in A has lower internal energy.(b) MA has lower specific heat and the water in B has higher internal energy.(c) MB has lower specific heat but the water in A and B have the same internal energy.(d) MB has higher specific heat but the water in A has higher internal energy.(e) MB and MB have the same specific heat and the water in A and B have the same internal energy.
- The process of heat radiation is the ONLY method of heat transfer that can occur under water.through space.through the air.through a solid.1. (a) How much heat transfer is necessary to raise the temperature of a 0.26 -kg piece of ice from -20 °C to 130 °C, including the 20 kJ/s energy needed for phase changes? Specific heat of ice = 2.090 kJ/kg °C Specific heat of water = 4.186 kJ/kg °C Specific heat of steam = 1.520 kJ/kg °C Heat of fusion of water = 334 kJ/kg Heat of vaporization = 2256 kJ/kg (i) Heat needed to warm ice to 0 °C: Q₁: ✔KJ (ii) Heat needed to melt ice at 0 °C: Q₂: KJ (iii) Heat required to warm 0 °C water to 100 °C: Q3: KJ (iv) Heat required to vaporize water at 100 °C: Q4: KJ (v) Heat required to warm 100 °C vapor to 130 °C: Q5: KJ Total heat, Q: KJ (b) How much time is required for the entire process, assuming a constant 20.0 kJ/s rate of heat transfer? Total time, t: SA small chunk of dry ice (solid carbon dioxide) at 195 K is added to a thermally insulatedcontainer filled with liquid nitrogen at its boiling point of 77 K. What happens in thecontainer?(A) The dry ice melts until thermal equilibrium is established.(B) Some of the liquid nitrogen boils and the dry ice gets colder.(C) Some of the liquid nitrogen freezes and the chunk of dry ice gets larger.(D) An equilibrium temperature is reached without any phase changes occurring.