A 4.00 kg silver ingot is taken from a furnace at 750.0°C andplaced on a large block of ice at 0.0°C. Assuming that all the heat givenup by the silver is used to melt the ice, how much ice is melted?
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A 4.00 kg silver ingot is taken from a furnace at 750.0°C and
placed on a large block of ice at 0.0°C. Assuming that all the heat given
up by the silver is used to melt the ice, how much ice is melted?
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- The American Burn Association states 3. You heat up an aluminum sphere of radius r, 1.27254 cm to 100 °C. You cool a 20.0 g copper ring to 0.00000 °C. The inner radius of the copper ring is r, 1.27000 cm. You then place the sphere on top of the ring and they are allowed to reach thermal equilibrium. Assume no heat loss to the surroundings. At the equilibrium temperature the sphere falls through the ring. (a) What is the thermal equilibrium temperature? (b) What was the amount of heat that was transferred between the ring and the sphere? (e) Which object lost the heat and which object gained the heat? (d) What is the mass of the aluminum sphere? Do not use the definition of density to solve for the mass. OWhat minimum heat is needed to bring 100 g of water at 40 ∘C to the boiling point and completely boil it away? The specific heat of water is 4190 J/(kg⋅K) and its heat of vaporization is 22.6××1055 J/kg. Express your answer with the appropriate units.A 23 g ice cube at -15.0oC is placed in 129 g of water at 48.0oC. The Specific heat of ice is 2.090 J/g K, the specific heat of water is 4.186 J/g K, and the latent heat of fusion for water is 333 J/g. What is final temperature in celsius of the system when the equilibrium is reached. Ignore the heat capacity of the container and assume this is in a calorimeter.
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