Question

a 25.0-g sample of ice at -6.5oc is removed from the freezer and allowed to warm until it melts. given the data below, select all the options that correctly reflect the calculations needed to determine the total heat change for this process. melting point at 1 atm

Answer 1

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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