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25.0 gg of copper pellets are removed from a 300∘C∘C oven and immediately dropped into 80.0 mLmL of water at 25.0 ∘C∘C in an insulated cup
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- Suppose 26.0 g of neon gas are stored in a tank at a temperature of 152C. (a) What is the temperature of the gas on the Kelvin scale? (See Section 10.2.) (b) How many moles of gas are in the tank? (See Section 10.4.) (c) What is the internal energy of the gas? (See Section 10.5.)Consider the latent heat of fusion and the latent heat of vaporization for H2O, 3.33 105 J/kg and 2.256 106 J/kg, respectively. How much heat is needed to a. melt 2.00 kg of ice and b. vaporize 2.00 kg of water? Assume the temperatures of the ice and steam are at the melting point and vaporization point, respectively. (a). UsingEq21.9, Q = mLF = (2.00 kg) (3.33l05 J/kg) = 6.66105 J (b).UsingEq21.10. Q = mLV = (2.00kg) (2.256106 J/kg) = 14.51106 J22.0 gg of copper pellets are removed from a 300∘C∘C oven and immediately dropped into 80.0 mLmL of water at 25.0 ∘C∘C in an insulated cup. What will the new water temperature be?
- A steam pipe is covered with 1.25 cm thick insulating material of thermal conductivity 0.200 W / m. ° C. How much energy is lost every second when the steam is at 200 ° C and the surrounding air is at 20 ° C? The pipe has a circumference of 950 cm and a length of 68 m. Neglect losses through the ends of the pipe.Estimate how long (in seconds) it should take to bring a cup of water to boiling temperature in a typical 700-watt microwave oven, assuming that all the energy ends up in the water. Something to think about: why is no heat involved in this process? The heat capacity of water is 75.29J/K/mol. A cup of water is about 250mL. Assume the water is at 25°C to start with (typical room temperature). Relative tolerance +/- 2% SA 50g ice cube at 0 0C is heated until 45ghas become water at 100 oC and 5g has become steam at100 oC . Determine the amount of heat that will be added to accomplish this [ Cwater =4186 Jkg_1 , Lv= 2.26*106 Jkg -1 , Lf = 3.133 *105 Jkg_1
- A steam pipe is covered with 1.50-cm thick insulating material of thermal conductivity of 0.200 cal/cm · °C · s. How much energy is lost every second when the steam is at 250°C and the surrounding air is at 20.0°C? The pipe has a circumference of 800 cm and a length of 64.0 m. Neglect losses through the ends of the pipe. ?MWHeat is needed to change 200 g of ice at 0°C to steam at 120°C?Cwater = 4186 J/kg.C⁰Cvapor = 2010 J/kg⋅C⁰Lf = 3.33 x 10⁵ J/kgLv = 2.26 x 10⁶ J/kg1. How much energy is required to melt 200 g of ice originally at 0⁰C? 2. How much energy is gained when the water warms to 100⁰C? 3. How much energy is gained when all the water at 100⁰C vaporizes? 4. How much is the total energy in joules that must be added to ice at 0°C to convert to steam at 120°C?A 400.0 gg chunk of an unknown metal, which has been in boiling water for several minutes, is quickly dropped into an insulating Styrofoam beaker containing 1.20 kgkg of water at room temperature (20.0∘C∘C). After waiting and gently stirring for 5.00 minutes, you observe that the water's temperature has reached a constant value of 22.0 ∘C∘C. Assuming that the Styrofoam absorbs a negligibly small amount of heat and that no heat was lost to the surroundings, what is the specific heat of the metal? Express your answer in Joules per kilogram-Kelvin.
- A 1.82 m wide by 1.11 m high metal plate must be insulated to prevent contact burn injuries. If the heat transfer rate is 136 W and the temperature across the insulation must be reduced from 87.3°C to 40.3°C, what is the minimum thickness (in cm) of insulation required [round your final answer to two decimal places]? {kins = 0.031 W/m∙K}A 2.5 kg lump of aluminum is heated to 96oC and then dropped into 9.0 kg of water at 5.1oC. Assuming that the lump–water system is thermally isolated, what is the system's equilibrium temperature? Assume the specific heats of water and aluminum are 4186 and 900 J/kg-K, respectively.A 405-g sample of lead with specific heat cPb = 128 J/(kg · °C) at 87.0°C and a 220-g sample of silver with specific heat cAg = 230.0 J/(kg · °C) at 38.0°C are added to 0.500 kg of water at 22.0°C where specific heat of water cW = 4190 J/(kg · °C) in an insulated container. Assuming the system is thermally isolated, what is its final equilibrium temperature?