An ice cube of mass 100 g and at 0 degree C is dropped into a Styrofoam cup cont

Question

An ice cube of mass 100 g and at 0 degree C is dropped into a Styrofoam cup containing 200 g of water at 25 degree C. Calculate how much heat is available by cooling the water to 0 degree C and how much heat is required to much the ice. L_f = 80 cal/g; c_ = 1.0 cal/g degree C Available Heat: Q_ = cal. Required heat: Q_ = cal Will all the ice melt? A certain amount of heat is transferred to a system, and the system performs some work on its surroundings. The amount of work done is less than the heat added. Thus the internal energy of the system increased. the internal energy of the system decreased. there has been a violation of the principle of conservation of energy. there must have been a phase change. The volume of an ideal gas is increased from 1 m^3 to 3 m^3 at a constant pressure of 1000 Pa How much work is done by the gas in the expansion? W = _______ J If no heat has been added or removed, what is the change in internal energy of the gas? Delta U = ______ J Work of 1500 J is done on an ideal gas, but the internal energy raises only 800 J. What is the amount and direction of the heat flow into or out of the gas? Q = _________ cal If 500 cal of heat is added to a gas, and the gas expands doing 500 J of work on its surroundings, what is the change in the internal energy of the gas? Delta U = ________ J Heat is added to an ideal gas and the gas expands. In such a process the temperature must always increase. will remain the same if the work done equals the heat added. will remain the same if work done is less than the heat added. will remain the same the work done exceeds the heat added. Which of the three processes of heat flow is most effective for: (a) A hot body in vacuum, e.g. a star like the the sun in space ________ (b) A hot liquid, e.g. outer iron-nickel core of the Earth ________ (c) A hot solid, e.g. the solid inner iron-nickel core of the Earth ________ Calculate the amount of heat to be added to warm 150 g of ice from -10 degree C to produce steam at 110 degree C? Ice: c_ice = 0.5 cal/g middot degree C, L_t = 80 cal/g; Water C_ = 1.0 cal/g middot degree C; Steam c_ = 0.5 cal/g middot degree C, L_ = 540 cal/g

Explanation / Answer

24)
Latent Heat of ice, Li = 80 cal/gm
Heat available by cooling the water to 0oC = m*cw*T = 200 * 1.0 * 25 = 5000 cal
Heat required to melt ice = m*Li = 100 * 80 = 8000 cal

As Heat required to melt ice > Heat available by cooling the water
Therefore,
All ice will not melt

25)
The first law of thermodynamics states,
U = Q - W

Given, W < Q
Therefore U will increase !!
The internal energy of the system increased !!

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