A 0.150-kg block of a pure material is heated from 20.0°C to 65.0°C by the addition of 2.18 kJ of energy. Calculate its specific heat. kJ/(kg · °C)
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- How much thermal energy (in J) is required to boil 2.75 kg of water at 100.0°C into steam at 157.0°C? The latent heat of vaporization of water is 2.26 ✕ 106 J/kg and the specific heat of steam is 2010 J kg · °C . HINT JA closed box is filled with dry ice at a temperature of -86.0 °C, while the outside temperature is 21.0 °C. The box is cubical, measuring 0.394 m on a side, and the thickness of the walls is 4.49 × 102 m. In one day, 3.76 × 106 J of heat is conducted through the six walls. Find the thermal conductivity of the material from which the box is made. Number UnitsA raindrop strikes the ground with a speed of 6.1 m/s. The specific heat of water is 4.19 × 103 J/(kg⋅°C). What is the raindrop’s change in temperature after it strikes the ground, in degrees Celsius, assuming all its initial kinetic energy goes into heating it?
- How much energy is required to change a 31 g ice cube from ice at -11 °C to steam at 112°C? The specific heat of ice is 2090 J/kg °C, the specific heat of water is 4186 J/kg °C and the specific heat of steam is 2010 J/kg °C. The heat of fusion of water is 333000 J/kg and the heat of vaporization is 2.26 × 106 J/kg. Answer in units of J.A classroom has dimensions 8.00 m x 10.00 m x 3.00 m. A 1000 W electric space heater is being used to warm the room from 5.00°C to 20.00°C on a cold morning. If the density of air is 1.29 kg/m°, and the specific heat capacity of air is 1004 J/(kg-K), how long will it take to heat the room? Assume no loss of thermal energy to the surroundings. A) 1.30 minutes B) 241 minutes C) 45.3 minutes O D) 77.7 minutesThe energy given off as heat by 310 g of an alloy as it cools through 40C° raises the temperature of 310 g of water from 30°C to 40° C. The specific heat of the alloy (in J/kg · C°) is: (Use c of water = 4186 J/kg C°) A surveyor’s 35-m steel tape is correct at 68° F. On a hot day the tape has expanded to 35.03 m. On that day, the tape indicates a distance of 16.50 m between two points. The true distance between these points is:
- A 900 g copper rod at 20 degrees celcius has a length of 1.0000 m. The thermal expansion coefficient of copper is 17 x 10^-6 degrees celcius -1. The specific heat capacity is 0.385 kJ/kg degrees celcius. Question A: The copper is heated to 400 degrees celcius. What is the new length? Give the answer in meters and with 4 digits of precision after the decimal. Question B: The hot copper is then quenched by dunking the entire rod in a bucket with 10 kg of water at 20 degrees celcius. The specific heat capaciy of water is 4.18 kJ/kg degrees celcius. If none of the water turns to steam what is the equilibrium temp of the copper rod and water? Please give the answer in degrees celcius Question C: You measure the equilbrium temp and find that it is 24 degrees celcius. If the latent heat of vaporization of water is 2,260 kJ/kg, what mass of water turned to steam? Answer in gramsA copper cylinder with a mass of 125 grams and a temperature of 345 ° C cools when placed in a glass container containing 565 g of water initially at 20.0 ° C. The mass of the container is 50.0 g and the specific heat of the glass is 840 J / kg ∙ K. What is the temperature of the system when it reaches thermal equilibrium? assuming that the cooling occurs very quickly, so that no energy is lost in the air. The specific heat of copper is 385 J / kg ∙ K and that of water is 4190 J / kg ∙ K.A 20.0 g ice cube is 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 L=79.5 cal/g. Specific heat for water is 1.00 cal/gK, and for ice 0.530 cal/gK. 10.1 O 13.2 1.83 0.00 none of them
- In an experiment, you need to cool a 0.25 kg of water from 25 °C to 0 °C. How much ice (initially at -20 °C) should you completely melt into the water to obtain your target temperature. The heat capacity of the container may be neglected. Cice = 2100 J/kg·K Cwater = 4186 J/kg·K Lf for water = 33.5x104 J/kgA 0.0550 kg ice cube at −30.0°C is placed in 0.577 kg of 35.0°C water in a very well insulated container. What is the final temperature? The latent heat of fusion of water is 79.8 kcal/kg, the specific heat of ice is 0.50 kcal/(kg · °C), and the specific heat of water is 1.00 kcal/(kg · °C). Answer in degrees Celcius.When 345 g of water at 35.0 °C and 295 g of water at 63.0 °C are added together in a calorimeter, the temperature of the mixture becomes 46.9 °C. If the specific heat capacity of water is 4.18 J/g °C, how many kilojoules of energy are absorbed by the calorimeter?