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Iron has a specific heat that is about 3.4 times that of gold. A cube of gold and a cube of iron, both of equal mass and at 20 °C, are placed in two different Styrofoam cups containing water each at 40 °C and having negligible heat transfer. After equilibrium is obtained, which one has a higher temperature? Explain

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#6. My buddy is starting to get hypothermic (body temperature 306 K) during an epic backcountry ski adventure. Since I'm quite warm (body temperature 310 K), I decide to get in a sleeping bag with him to try and warm him up. What heat transfer mechanism will be most responsible for heating him up? For simplicity, ignore any internal temperature differences across my body (that is, assume my skin temperature is also 310 K). Use num- bers to support your answer (for human skin, you can use the following values: surface area A = 1.50 m², emissivity = 0.970, thickness d= 0.0250 m, thermal conductivty 0.200 ms.K)
A styrofoam cooler (k = 0.030 W/(m-°C) has outside dimensions of 0.170 m x 0.250 m x 0.260 m, and an average thickness of 2.0 cm. How long will it take for 1.10 kg of ice at -5.0°C to melt (to water at 0°C) in the cooler if the outside temperature is 34.0°C? Assume that ice temperature increases linearly from -5.0°C to 0°C. Neglect any temperature change of the air in the cooler. Data: Specific heat of ice is 2050 J/(kg-K). Laten heat of fusion of water is 3.34×105 J/kg.
#6. My buddy is starting to get hypothermic (body temperature 306 K) during an epic backcountry ski adventure. Since I'm quite warm (body temperature 310 K), I decide to get in a sleeping bag with him to try and warm him up. What heat transfer mechanism will be most responsible for heating him up? For simplicity, ignore any internal temperature differences across my body (that is, assume my skin temperature is also 310 K). Use num- bers to support your answer (for human skin, you can use the following values: surface area A = 1.50 m², emissivity € = 0.970, thickness d = 0.0250 m, thermal conductivty 0.200 ms.K) J
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.
The same amount of heat entering identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.70 kcal of heat enters 1.38 kg of the following, originally at 30.2°C. The specific heat capacity for each material is given in square brackets below. (a) water [1.00 kcal/(kg · °C)] °C (b) concrete [0.20 kcal/(kg · °C)] °C (c) steel [0.108 kcal/(kg · °C)] °C (d) mercury [0.0333 kcal/(kg · °C)] °C
The same amount of heat entering identical masses of different substances produces different temperature changes. Calculate the final temperature when 1.40 kcal of heat enters 1.83 kg of the following, originally at 28.2°C. The specific heat capacity for each material is given in square brackets below. (a) water [1.00 kcal/(kg · °C)] °C (b) concrete [0.20 kcal/(kg · °C)] °C (c) steel [0.108 kcal/(kg · °C)] °C (d) mercury [0.0333 kcal/(kg · °C)] °C
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.
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: S