The answer is 53.8 kJ. Solution:There are two major steps in converting ice to liquid water. It begins with a phase change when ice melts at 0.0°C, and then a temperature change when the liquid water rises in temperature from zero to 32°C. The amount of heat involved with the phase change melting is given by q = (mass of water) (ΔHfus) = (115.0 g)(334 J/g) = 38410 J = 38.41 kJ The amount of heat involved with temperature change is q = mcΔT = (115.0g)(4.184J/g°C)(32°C - 0.0°C) = 15397.12 J = 15.39712 kJ Summing up the two values gives the total heat required to convert ice to liquid water: q = 38.41 kJ + 15.39712 kJ= 53.8 kJ
The best and most correct answer among the choices provided by your question is the fourth choice.
Copper <span>has an average atomic mass of about 63.5 </span>amu<span>.</span>
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