In a nuclear power plant, a 1.0 kg of water at 56.9 °C is converted into 1.0 kg of steam at 154.7 °C. The total heat (in kcal) supplied by the plant is
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In a nuclear power plant, a 1.0 kg of water at 56.9 °C is converted into 1.0 kg of steam at 154.7 °C. The total heat (in kcal) supplied by the plant is
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- Beryllium has roughly one-half the specific heat of water (H2O). Rank the quantities of energy input required to produce the following changes from the largest to the smallest. In your ranking, note any cases of equality, (a) raising the temperature of 1 kg of H2O from 20C to 26C (b) raising the temperature of 2 kg of H2O from 20C to 23C (c) raising the temperature of 2 kg of H2O from 1C to 4C (d) raising the temperature of 2 kg of beryllium from 1C to 2C (e) raising the temperature of 2 kg of H2O from -1C to 2CThree 20.0 g ice cubes are dropped into 200 g of water in a thermally insulated container. If the water is initially at 20.0°C, and the ice comes directly from a freezer at -18.0°C, what is the final temperature in °C at thermal equilibrium? Heat of transformation for ice is LF-79.5 cal/g. Specific heat for water is 1.00 cal/gK, and for ice 0.530 cal/gK.A 75.0-g cube of ice at −10.0°C is placed in 0.620 kg of water at 50.0°C in an insulating container so that no heat is lost to the environment. Specific heat capacity (15.0°C) of water is 4.186 kJ/(kg·K) and that of ice (0°C) is 2.10 kJ/(kg·K) and heat of fusion of water is 333.7 kJ/kg. A) What will be the final temperature of this system? in c i asked how to do this but got the wrong solotion
- A 75.0-g cube of ice at −10.0°C is placed in 0.610 kg of water at 50.0°C in an insulating container so that no heat is lost to the environment. Specific heat capacity (15.0°C) of water is 4.186 kJ/(kg·K) and that of ice (0°C) is 2.10 kJ/(kg·K) and heat of fusion of water is 333.7 kJ/kg. What will be the final temperature of this system?A 10 kg of ice at 0 °C is mixed with 4 kg of steam at 100 °C in a thermally isolated container and allowed to reach thermal equilibrium. What is the amount of heat needed to melt the ice? The latent heats of fusion and vaporization of water is 334000 J/kg and 2256000 J/kg, respectively and the specific heat of liquid water is 4186 J/kg.K.1.2-kg of ice at -6.0°C is dropped into 5.0 L (5.566-kg) of car coolant. The initial temperature of the coolant is 25.0°C. The ice and coolant are insulated, so energy transfers to the outside is negligible. After hours, all ice melts and the final temperature of the mixture of water-coolant is 1.8°C. The specific heat of ice is 2090 J/kg °C; the specific heat of water is 4186 J/kg °C; the latent heat of fusion for water is 334000 J/kg. A. What is the energy needed for heating the ice to 0 °C? B. Determine the energy needed to melt the ice into water. C. Determine the total energy needed to heat the -6.0°C ice to 1.8°C water. (Please note: the total energy also includes the part heating water from 0.0 °C to 1.8 °C.) D. Determine the specific heat capacity of the coolant.
- The concrete slab of a basement is 11m long, 8 m wide and 0.2 m thick. During the winter, temperatures are nominally 17°C and 10°C at the top and bottom respectively. If the concrete has thermal conductivity of 1.4 W/m K, what is the rate of heat loss through the slab? If the basement is heated by a gas furnace operating at an efficiency of 90% using natural gas priced at Cg = Php 1.00/MJ, what is the daily cost of heat loss?One way to keep the contents of a garage from becoming too cold on a night when a severe subfreezing temperature is forecast is to put a tub of water in the garage. If the mass of the water is 122 kg and its initial temperature is 24.2°C, how much energy must the water transfer to its surroundings in order to freeze completely? The specific heat of water is 4186 J/kg·K, and the latent heat of fusion is 333 kJ/kg.A 0.250-kg aluminum bowl holding 0.800 kg of soup at 28.0°C is placed in a freezer. What is the final temperature if 430 kJ of energy is transferred from the bowl and soup? Assume the soup has the same thermal properties as that of water, the specific heat of the liquid soup is 1.00 kcal/(kg · °C), frozen soup is 0.500 kcal/(kg · °C), and the latent heat of fusion is 79.8 kcal/kg. The specific heat of aluminum is 0.215 kcal/(kg · °C). °C
- A 0.250-kg aluminum bowl holding 0.800 kg of soup at 25.0°C is placed in a freezer. What is the final temperature if 430 kJ of energy is transferred from the bowl and soup? Assume the soup has the same thermal properties as that of water, the specific heat of the liquid soup is 1.00 kcal/(kg · °C), frozen soup is 0.500 kcal/(kg · °C), and the latent heat of fusion is 79.8 kcal/kg. The specific heat of aluminum is 0.215 kcal/(kg · °C).You mix mI = 1.2 kg of ice at TI = -21°C with mW = 4.8 kg of water at TW = 72°C in an insulated container. The specific heats of ice and water are cI = 2.10×103 J/(kg⋅°C) and cW = 4.19×103 J/(kg⋅°C), respectively, and the latent heat of fusion for water is Lf = 3.34 × 105 J/kg. Enter an expression for the final equilibrium temperature of the mixture in terms of the defined quantities.How much thermal energy is required to boil 4.11 kg of water at 100.0°C into steam at 132 °C? Properties of water you might find useful: density = 1000 kg / m , specific heat = 4186 J / (kg · °C), the latent heat of fusion = 3.33 x 105 J / kg, the latent heat of vaporisation = 2.26 x 106 J / kg, and the specific heat of steam = 2010 J / (kg · °C).
