A 15.7 g aluminum block is warmed to 53.2 deg C and plunged into an insulated beaker containing 32.5 g of water initially at 24.5 deg C.  The aluminum and the water are allowed to come to thermal equilibrium.  Assuming that no heat is lost, what is the final temperature of the water and aluminum?

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A: I  Answerd question 2 and it's all part ,  please post next question separately.

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A: 150 kJ of heat is released from the system

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A: Given data,

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A: From the formula of specific heat capacity we have solved this problem.

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Q: If a system does 73.0 kJ of work on its surroundings and releases 105 kJ of heat, what is the change…

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Q: A system receives 315J of heat and delivers 200. J of work to its surroundings, what is the change…

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Q: When thermal energy is transferred from the system to its surroundings, heat (q) is:

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A: There are two types of processes defined based on the heat transfer  1) Exothermic  2) Endothermic

Q: How many Joules of energy would be required to heat 35g of water from 23C to 29C?

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A: For this problem We have to find the change in internal energy for the given condition.

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Q: A hot lump of 42.4g of copper at an initial temperature of 64.7 °C is placed in 50.0 mL H2O…

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Q: A piece of copper alloy with a mass of 85.0g is heated from 30.0°C to 45.0°C. In the process, it…

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A: Thermodynamics is the study of heat in motion.

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