If say 70 mL of water is heated vs 100 mL of water, would the temperature be different or does the amount of the substance not make a difference on the temperature
Thanks!
Never mind, I figured out that it shouldn't make a difference. That's what I originally thought, but just wanted to clarify.
It could make a difference depending upon how the question is stated.
If you add the SAME AMOUNT of heat(in calories or joules) to a 70 mL sample vs a 100 mL sample, then the 70 mL will have a higher temperature.
The amount of a substance, in this case, water, does not affect the temperature reached when heating it. According to the basic principles of thermodynamics, the temperature of a substance is determined by the amount of energy (in this case, heat) transferred to it, rather than the volume or quantity of the substance.
When you heat a substance, the energy is used to increase the kinetic energy of its molecules, thus raising the temperature. The quantity of water molecules in a given volume (e.g., 70 mL or 100 mL) does not affect their ability to absorb heat or increase their kinetic energy.
However, it's worth noting that larger volumes of water will generally require more heat energy input to raise their temperature compared to smaller volumes. But if you provide the same amount of energy (e.g., by using the same heat source for both 70 mL and 100 mL of water), the temperatures reached by both volumes will be the same.
In summary, the temperature reached when heating water is primarily determined by the amount of heat energy supplied, rather than the quantity or volume of the water itself.