The convert ice at -100c to 00C
q1 = mcT
= 25*2.09*(0-(-10)
= 25*2.09*10
= 522.5J
The fusion of ice
q2 = mH fusion
= 25*334 = 8350J
The water convert at 00C to 1000C
q3 = mcT
= 25*4.184*(100-0) = 10460J
The heat of vaporization of water
q4 = mH
= 25*2257 = 56425J
The steam convert 1000C to 1100C
q5 = mcT
= 25*2.09*(110-100) = 522.5J
The total heat energy changes
q = q1 + q2 + q3 + q4 + q5
= 522.5 + 8350 + 10460 + 56425 + 522.5
= 76280J
= 76.28KJ >>>>answer
Part 2: Multi-Step Curves (Day 2) 1. How much energy (in kJ) is required to get a 25.0 g ice cube (water) at -10.0...
3. How much energy (in kJ) is required to get a 100. g ice cube at -10.0°C to completely melt? (HINT: Which AH andispecific heat (e) are used for melting solid to a liquid?)
1. How much energy (in kJ) is required to completely vaporize 200.g of 25.0*C liquid water? Step 1: How much energy does it take to get the water from 25.00°C to boiling? This where you use Qumc(TFT) because this part is just a heat flow problem, not a phase change like the next part.
014 10.0 points How much energy is required to change a 35 g ice cube from ice at -12°C to steam at 111°C? The specific heat of ice is 2090 J/kg.° C, the specific heat of water is 4186 J/kg.° C, the specific heat of stream is 2010 J/kg.° C, the heat of fusion is 3.33 x 10° J/kg, and the heat of vaporization is 2.26 × 106 J/kg. Answer in units of J
2. How much energy (in kJ) is released when a 75.0 g of water vapor at 125°C forms an ice cube at -5.50°C? HINT: it still has to go through all of the same steps, even if they are not listed like in the last problem.
How much energy (heat) is required to convert 52.0 g of ice at -10.0 C to steam at 100 C?Specific heat of ice: 2.09 J/g * C DHfus = 6.02 kJ/molSpecific heat of water: 4.18 J/g * C DHvap = 40.7 kJ/molSpecific heat of steam: 1.84 J/g * C
a. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g of liquid ethanol from -5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid= 2.46J/g°C AHvap=38.6 kJ/mol b. How much heat (kJ), at 1 atm, is required to raise the temperature of 25.0 g water from 5.0°C to its boiling temperature and then vaporize all of it? Cs, liquid=4.184 /g°C AHvap=40.7 kJ/mol
Part A: How much heat energy, in kilojoules, is required to convert 76.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. Part B: How long would it take for 1.50 molmol of water at 100.0 ∘C∘C to be converted completely into steam if heat were added at a constant rate of 17.0 J/sJ/s ?
How much heat (in kJ) is required to warm 10.0 g of ice, initially at -10.0 ∘C, to steam at 112.0 ∘C? The heat capacity of ice is 2.09 J/g⋅∘C and that of steam is 2.01 J/g⋅∘C.
PART A How much heat energy, in kilojoules, is required to convert 62.0 g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to three significant figures and include the appropriate units. part B How long would it take for 1.50 mol of water at 100.0 ∘C to be converted completely into steam if heat were added at a constant rate of 23.0 J/s ? Express your answer to three significant figures and include the...
how much heat does it take to completely vaporize a 75.0g ice cube? given: ice = 0°C T boiling point = 100°C C water = 1cal/g°C Lf = 80.0 cal/g Lv = 540.0 cal/g