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Answer 1 · 2017-05-17T23:33:10

The substance is most likely iron.

It looks as if we should calculate the specific heat capacity of the substance.

The formula for the amount heat $q$ $q$ absorbed by a substance is

$color(blue)(bar(ul(|color(white)(a/a)q = mCΔTcolor(white)(a/a)|)))" "$

where

$m$ is the mass of the substance
$C$ is the specific heat capacity of the material
$ΔT$ is the temperature change

You can rearrange the formula to calculate the specific heat capacity:

$C = q/(mΔT)$

In this problem,

$q = 1.539 × 10^2color(white)(l) "J"$
$m = "17.1 g"$
$ΔT = "(45.0 - 25.0) °C" = "20.0 °C"$

∴ $C = (1.539 × 10^2color(white)(l) "J")/"17.1 g × 20.0 °C" = "0.450 J·°C"^"-1""g"^"-1"$

The Engineering Toolbox lists the following specific heat capacities of metals:

$"Cr = 0.46 kJ/(K·kg)"$
$"Fe = 0.45 kJ/(K·kg)"$
$"Ni = 0.44 kJ/(K·kg)"$

I will go for the one in the middle and say that the substance is most likely iron.