Question

Loren has the samples of elements that are listed below at room temperature. He exposes the samples to the same heat source until each sample reaches a temperature of 90.0°C. 10 g of Al(s) (mc003-1.jpg = 0.897 J/(gi°C)) 10 g of Ag(s) (mc003-2.jpg= 0.234 J/gi°C ) 10 g of Fe(s) (mc003-3.jpg = 0.450 J/gi°C) 10 g of Zn(s) (mc003-4.jpg = 0.387 J/gi°C ) From first to last, which lists the order in which these samples will reach 90.0°C? Al, Fe, Zn, Ag Ag, Zn, Fe, Al Al, Fe, Ag, Zn Ag, Al, Zn, Fe

Answer 1

Given:

Specific Heat (c) values :-

Al = 0.897 J/gC

Ag = 0.234 J/gC

Fe = 0.450 J/gC

Zn = 0.387 J/gC

Mass of all element = 10 g

Initial temperature T1 = 25 C

Final temperature T2 = 90 C

To determine:

The order in which the elements will reach 90 C

Explanation:

The heat (Q) absorbed by the elements is mathematically expressed as:

Q = mcΔT

where: m = mass of the substance

c = specific heat, which is the amount of heat required to raise the temperature of a unit mass of the substance by a unit degree

ΔT = change in temperature

In the given examples, m = 10 g for all elements and ΔT = 90-25 = 65 C is also the same

Therefore, the heat absorbed (Q) will depend only on the specific heat of the elements. Lower the value of the specific heat, lower is the amount of heat required to raise the temperature to 90 C and the element will heat up faster.

Based on the values of the specific heats, the order in which the samples would reach 90 C from the first to the last would be:

Ag, Zn, Fe, Al

Answer 2

Answer:

B. Ag, Zn, Fe, Al

Explanation:

this is correct on ed-genuity, hope this helps! :)