Select true or false: 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 2.42 times greater than that of the iron.

false.

Explanation:

1) The increase of temperature is calcualte with the formula:

Q = M × C × ΔT.

2) In this case, you can write:

For water: Qw = Mw × Cw × ΔTw

For iron: Qi = Mi × Ci × ΔTi

3) Since the heat absorbed and the masses are equal, you get:

Qw = Qi ⇒ Cw×ΔTw = Ci×ΔTi, from where you can clear ΔTw

4) ΔTw = Ci×ΔTi / Cw

Replacing the values: ΔTw = 0.444 ΔTi / 4.18 ≈ 0.11 ΔTi.

5) Conclusion the temperature increase of water will be 0.11 times the increase of temperature of iron (this is smaller). So, the statement is false.

hey your not cool]      

the dependant variable is spilled water

the independent is the heat