Part A.
Energy required to phase change is given by:
Q = m*Lf
m = mass of water = 1 gm = 1*10^-3 kg
Lf = Latent heat of fusion = 3.337*10^5 J/kg
So,
Q = 1*10^-3 kg*(3.337*10^5 J/kg)
Q = 3.337*10^2 J = 333.7 J
Correct option is C. (See that SI unit of heat is J and not J/kg, So that must be a typo error)
2.
Increase in Volume of due to change in temperature is given by:
dV = V0**dT
Here, = Volumetric expansion coefficient of aluminum = 70*10^-6 /C (Again in the question there is typing error, as we know that = 3, So it is 100% 10^-6 and 10^9)
Now dT = change in temperature = 575 C
So,
dV = V0*70*10^-6*575
dV = V0*0.04025
dV/V0 = 0.04025
In percentage terms
dV/V0 = 4.025%
Volumetric change of the cube is 4.025%
Let me know if you've any query.
What mass of ice would it take to lower the temperature of 0.5kg of water 20°C to 0°C. 7. from A 100-g piece of iron is heated to 100°C and then dropped into a cavity in a large block ofice at 0°C. How much mass of ice will melt? 8. 50 grams of hot water at 80°C is poured into a cavity in a very large block ofice at 0°C. The final temperature of the water in the cavity is...
2. How much heat transfer is necessary to raise the temperature of a 0.500 kg piece of ice from -30.0C to 110.0 C? cice-2090 J/kg C, Cater 4186 J/kg C,Cseam 1520 J/kg C, L-334 kJ/kg and Lv-2256 kJ/kg. 2. How much heat transfer is necessary to raise the temperature of a 0.500 kg piece of ice from -30.0C to 110.0 C? cice-2090 J/kg C, Cater 4186 J/kg C,Cseam 1520 J/kg C, L-334 kJ/kg and Lv-2256 kJ/kg.
How much heat, in kcal, does it take to melt a 500 gram block of ice originally at 0.0 C until it is liquid water at 25.0 C? Please show work. Thank you!
How much heat is required to change a 50.0 g ice cube from ice at -10.7°C to water at 62°C? (if necessary, use cice=2090 J/kg°C and csteam= 2010 J/kg°C) How much heat is required to change a 50.0 g ice cube from ice at -10.7°C to steam at 113°C?
How much heat is required to change a 47.4 g ice cube from ice at -11.8°C to water at 68°C? (if necessary, use cice=2090 J/kg°C and csteam= 2010 J/kg°C) How much heat is required to change a 47.4 g ice cube from ice at -11.8°C to steam at 115°C?
How much heat is required to change 456 g of ice at -20.0Degree C into water at 25.0Degree C? specific heat of water = 4186]/(kg-K); specific heat of ice = 2090 J/(kg.K) and latent heat of fusion of water = 33.5 times 10^4 J/kg.
The specific heat of water is 4186 J/kg C. How much does the internal energy of 300 grams of water change as it is heated from 23 to 46 degrees C? Assume that the volume is constant. Internal energy change = Number Joules
How much heat is needed to take a 64.9 gram block of ice from -22.2o C to 22.2o C? Answer in Calories to 3 significant figures.
How much heat must be added to a 8.0-kg Nock of ice at -8 degree C to change it to water at 14 degree C? The specific heat of ice is 2050)/kg middot C degree. the specific heat of water is 4186 J/kg middot C degree, the latent heat of fusion of ice is 334,000 J/kg. and 1 cal = 4.186 J. A) 140 kcal B) 780 kcal C)730kcal D)810kcal E) 180 kcal
How much heat is required to warm to 0 degrees C and then melt a 100ml block of ice( at 20 degrees C) that is 100ml in volume? Density of ice is 0.92 g/ml. DeltaHfus=6.01 kJ/mol. DeltaHvap=44kj/mol. Heat capacity of ice= 2.09 j/g C. Heat capacity of water= 4.184 J/g C.