Answer:
Ag(s), Zn(s), Fe(s), Al(s).
Explanation:
Specific heat capacity is defined as the amount of heat energy required to raise the temperature of a substance per unit of mass. In the problem, you have specific heat of each sample:
Al(s) = 0.897 J/(g°C)
Ag(s) = 0.234 J/(g°C)
Fe(s) = 0.450 J/(g°C)
Zn(s) = 0.387 J/(g°C)
As the mass of the samples is the same, the compound that reach first the temperature is the one with less specific heat capacity. Thus, order is:
Ag(s), Zn(s), Fe(s), Al(s).
Answer:
Ag>Zn>Fe>Al
Explanation:
Step 1: Data given
Final temperature = 90.0 °C
10 g of Al(s) ( = 0.897 J/(g°C))
10 g of Ag(s) (= 0.234 J/g°C )
10 g of Fe(s) ( = 0.450 J/g°C)
10 g of Zn(s) ( = 0.387 J/g°C )
Suppose the initial temperature is 0 °C
Step 2: Calculate the heat needed to heat
Q = m*C*ΔT
⇒with Q = the heat needed to heat the elements
⇒with m = the mass of the sample = since the mass is the same for each sample, this will not affect
⇒with c = the specific heat of the sample = the heat needed to raise 1 gram of the sample 1°C
⇒ΔT = the change of temperature = since all of the sample have the same initial and final temperature, this will not affect.
The sample with the lowest specific heat capacity will reach 90.0 °C the first
10 g of Ag(s) will heat the fastest
10 g of Zn(s)
10 g of Fe(s)
10 g of Al(s)
Ag>Zn>Fe>Al
