What would the effect on the specific heat of your metal if one drop (0.05mL) of water at 100 degrees Celsius remained on your metal? the effect would cause the specific heat to be much higher none of these choices are correct the effect would cause the specific heat to be much lower the effect would be negligible

In the above image, you have a solid at less than 0 oC. As you add heat (Q), the temperature of the solid increases until it hits a point when it would start melting. In the case of water, this is at 0 oC. Notice that at this point the temperature stops rising and we have a mixture of solid/liquid. We are still adding heat but the temperature is not changing. Once all of our solid becomes liquid, the temperature starts to rise again until it hits another plateau, at 100 oC. This is the point where the water boils and starts becoming a gas. Again, we add heat but the liquid/gas mixtures temperature does not change. Once all the liquid has become gas, the temperature will start to rise again. Is it possible to have 0 oC water and 0 oC ice?   Yes or No?

If the same amount of heat is added to 5.00 g samples of each of the metals below, which metal will experience the largest temperature change?   Metal Specific Heat Capacity (J/g-K) A 0.753 B 0.129 C 0.385 D 0.449 E 0.897

How much heat is needed to raise the temperature of a 2.5 g piece of copper wire from 20. °C to 80. °C? How much heat is needed to increase the temperature of an equivalent mass of aluminum by the same amount? Once heated, which metal will cool faster?