The specific heat of water is 4.184 J/g degree C, and the specific heat of iron is 0.451 J/g degree C, which will reach a higher temperature when exposed to a given amount of heat?
It looks like water will absorb much more heat as it rises the same temperature.
To determine which substance will reach a higher temperature when exposed to a given amount of heat, we need to compare their specific heat values.
The specific heat of a substance is the amount of heat energy required to raise the temperature of one gram of that substance by one degree Celsius.
In this case, we have water with a specific heat of 4.184 J/g°C and iron with a specific heat of 0.451 J/g°C.
To calculate the heat energy required to raise the temperature of a substance, we can use the formula:
Heat energy (Q) = mass (m) × specific heat (c) × change in temperature (ΔT)
Let's assume we have the same mass of both water and iron and we provide the same amount of heat energy to both substances.
Since the specific heat of water (4.184 J/g°C) is higher than the specific heat of iron (0.451 J/g°C), water will require more heat energy to raise its temperature by 1 degree Celsius compared to iron.
Therefore, if we apply the same amount of heat energy to both substances, the water will reach a lower temperature compared to iron because it needs more heat energy per gram to be heated.
In conclusion, iron will reach a higher temperature when exposed to a given amount of heat compared to water.