Question

heat is a form of energy related to the motion, or kinetic energy, of the particles in a substance. when a substance absorbs heat energy, the temperature of the substance increases. the temperature change (δt) is dependent upon how much of the substance (mass) is present and the specific heat (sh) of the substance. the formula relating heat, mass, specific heat, and temperature change is heat = mass × sh × δt the following table lists the specific heats of some common substances: substance specific heat j/(g·°c) aluminum (al) 0.897 copper (cu) 0.385 cast iron 0.460 gold (au) 0.129 silver (ag) 0.235 sodium chloride (nacl) 0.864 stainless steel 0.500 water (h₂o) 4.184 part a rank the following species according to the decreasing energy needed to raise the temperature of 10.0 g of the substance by 25.0°c. rank from most to least energy needed. to rank items as equivalent, overlap them. view available hint(s)

Explanation:

Step1: Analyze the formula

The formula for heat is \(heat = mass\times SH\times\Delta T\). Here, \(mass = 10.0\ g\) and \(\Delta T=25.0^{\circ}C\) are constant. So the heat (energy) needed is directly proportional to the specific heat (\(SH\)).

Step2: Compare specific heats

From the table:

• \(SH_{water}=4.184\ J/(g\cdot^{\circ}C)\)
• \(SH_{aluminum}= 0.897\ J/(g\cdot^{\circ}C)\)
• \(SH_{stainless\ steel}=0.500\ J/(g\cdot^{\circ}C)\)
• \(SH_{copper}=0.385\ J/(g\cdot^{\circ}C)\)
• \(SH_{gold}=0.129\ J/(g\cdot^{\circ}C)\)

Since \(4.184>0.897 > 0.500>0.385>0.129\)

Answer:

water, aluminum, stainless steel, copper, gold