The specific heats of water and iron are 4.184 and 0.444 J/g°C, respectively.When equal masses of water and iron both absorb the same amount of heat, the temperature increase of the water will be 5.42 times greater than that of the iron.

Question

Quizplus · Accepted Answer

Let's assume that the equal masses of water and iron are m, and the amount of heat absorbed by both is Q.

Therefore, according to the formula for the heat absorbed by a specific substance:

Q = m × c × ΔT

where Q is the amount of heat absorbed, m is the mass of the substance, c is its specific heat capacity, and ΔT is the temperature change.

Since both water and iron absorb the same amount of heat (Q), we can set up an equation:

m × 4.184 × ΔT_w = m × 0.444 × ΔT_i

where ΔT_w and ΔT_i are the temperature changes of water and iron, respectively.

Dividing both sides by m and simplifying:

ΔT_w = 0.106 × ΔT_i

This means that the temperature increase of water will be 0.106 times that of iron.

However, the question says that the temperature increase of water is 5.42 times greater than that of iron.

Therefore, the statement is false, and the answer is B.

The Specific Heats of Water and Iron Are 4