A chemist places a 100 g cube of each of the metals listed in the table on a separate hot plate. All of the
hot plates are identical. Each hot plate is set on medium heat, and all of the cubes have the same initial
temperature. Based on the specific heat values in the table, rank the metals in terms of how quickly they
will reach the target temperature of 80°C. Use "1" to indicate the fastest and "5" to indicate the slowest.
Fe: -
Al: 0
Cp (J/g•°C)
0.450
0.897
Substance
Fe(s)
Al(s)
Cu(s)
Sn(s)
Pb(s)
Cu:
0.385
0.227
Sn:
0.129
Pb:

The answer is the first option just took the test

They are all solids.

The correct answer is "false"

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.