How much total heat is required to transform 500.73 g of ice at 0.0000 ◦C into steam at 100.00 ◦C? (For water:Lf = 80.000 cal/g, c = 1.0000 cal/(g◦C), Lv = 540 cal/g
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How much total heat is required to transform 500.73 g of ice at 0.0000 ◦C into steam at 100.00 ◦C? (For water:
Lf = 80.000 cal/g, c = 1.0000 cal/(g◦C), Lv = 540 cal/g
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- One of a dilute diatomic gas occupying a volume of 10.00 L expands against a constant pressure of 2.000 atm when it is slowly heated. If the temperature of the gas rises by 10.00 K and 400.0 J of heat are added in the process, what is its final volume?One way to cool a gas is to let it expand. When a certain gas under a pressure of 5.00 106 Ha at 25.0C is allowed to expand to 3.00 times its original volume, its final pressure is 1.07 106 Pa. (a) What is the initial temperature of the gas in Kelvin? (b) What is the final temperature of the system? (See Section 10.4.)At 25.0 m below the surface of the sea, where the temperature is 5.00C, a diver exhales an air bubble having a volume of 1.00 cm3. If the surface temperature of the sea is 20.0C, what is the volume of the bubble just before it breaks the surface?
- A hollow aluminum cylinder 20.0 cm deep has an internal capacity of 2.000 L at 20.0C. It is completely filled with turpentine at 20.0C. The turpentine and the aluminum cylinder are then slowly warmed together to 80.0C. (a) How much turpentine overflows? (b) What is the volume of the turpentine remaining in the cylinder at 80.0C? (c) If the combination with this amount of turpentine is then cooled back to 20.0C, how far below the cylinders rim does the turpentines surface recede?How much thermal energy (in J) is required to boil 2.45 kg of water at 100.0°C into steam at 135.0°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 JHow much heat is needed to convert 10 kg of water at 10◦C to steam at 110◦C? Specific heat capacity of water = 4.186 kJ/kg◦C, Latent heat of vaporization of water = 2264 kJ/kg.
- How much thermal energy is required to boil 2.00 kg of water at 100.0°C into steam at 125°C? The latent heat of vaporization of water is 2.26 x 106 J/kg and the specific heat of steam is 2010 J/(kg ∙ °C).Calculate the heat in kJ for 9.98 g of ice at -75.0 oC heated to -38.0 oC with a specific heat capacity of 2.087 J/(g·oC).What mass of steam at 100°C must be mixed with 112 g of ice at its melting point, in a thermally insulated container, to produce liquid water at 23.0°C? The specific heat of water is 4186 J/kg·K. The latent heat of fusion is 333 kJ/kg, and the latent heat of vaporization is 2256 kJ/kg.
- One mole of water vapor at 346 K cools to 280 K. The heat given off by the cooling water vapor is absorbed by 10 mol of an ideal gas, and this heat absorption causes the gas to expand at a constant temperature of 273 K. If the final volume of the ideal gas is 24 L, determine its initial volume. The specific heat of water is 4186 J/kg °C and the latent heat of vaporization is 2.26 x 106 J/kg. Answer in units of 1.At atmospheric pressure, how much energy is required to heat 47.0 g of H2O(s) at -10.0◦C to H2O(g) at 129.0◦C? specific heat ice - 2093 J/kg C latent heat of fusion - 334*10^3 J/kg specific heat water - 4184 J/kg C latent heat of vaporization - 2260*10^3 J/kg specific heat vapor - 2010 J/kg C These values are approximate and fine to use. Please show all work.How many joules are needed to change 50g of ice at 0°C to steam at 120°C?The latent heat of fusion of ice is 3.35 x 10°J/kg; latent heat of vaporization of water is 2.26 x 10°J/kg. The specific heat capacities of ice; water, and steam, respectively, are 2093 J/(kg. K), 4186 J/(kg. K) and 2010 J/(kg. K). out of Select one: A. 50.68 kJ B. 63.96 kJ O C. 227.6 kJ D. 53.96 kJ E. 20.5 kJ F. 800.2 kJ G. 153.7 kJ H. 22.76 kJ
