A 405-g sample of lead with specific heat cpb = 128 J/(kg · °C) at 91.0°C and a 220-g sample of silver with Cag = 230.0 J/(kg · °C) at 36.0°C are added to 0.500 kg of water at 22.0°C where Cw = 4190 J/(kg °C) in an insulated container. Assuming the system is thermally isolated, what is its final equilibrium temperature? %3D
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- A lab instructor performs an experiment using an aluminum cup that contains 225 g of water and a 130 g copper stirrer, all initially at 27.0°C. (Note that the student wears insulated gloves when handling the stirrer.) The lab instructor then adds a sample of silver to the water. The sample has a mass of 446 g and is initially at a temperature of 85.0*C. After stirring the mixture until it reaches thermal equilibrium, the lab instructor measures a final temperature of 32.0°C. What is the mass (in g) of the aluminum cup? Need Help? ReadA 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?A 390-g metal container, insulated on the outside, holds 170.0 g of water in thermal equilibrium at 21.0°C. A 18.0-g ice cube, at -15.0°C, is dropped into the water, and when thermal equilibrium is reached the temperature is 12.0°C. Assume there is no heat exchange with the surroundings. The specific heat capacity of water is 4190 J/kg ∙ K, the specific heat capacity of ice is 2090 J/kg ∙ K and the heat of fusion is 3.34 × 105 J/kg. What is the specific heat capacity of the metal of the container?
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