Total heat change for this process is 8.70 kJ.
Q = mcΔT, where Q is the symbol for heat transfer, m is the mass of the substance, and ΔT is the change in temperature. The symbol c stands for specific heat and depends on the material and phase.
The ice will be warmed from -6.5 ºC to OºC where it will melt.
Lets q1 be the heat required to bring the ice to 0ºc, q₂ the heat required to bring the phase change from solid to liquid.
Given,
Mass of ice = 25 g
Change in temperature t = (0-(-6.5)) *C
Specific heat = 2.09 J/g *C
For heat q1 = m x c x t
= 25 g x 2.09 J/g C x 6.5
=339.626 J = 0.339 kJ
q2 = n x t (no of moles) x (molar heat of fusion of water)
= 25/18 mol x 6.02 kJ/mol
= 1.39 x 6.02 = 8.36 kJ
Total heat = q1 + q2
=8.36 + 0.339 = 8.70 kJ
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