What is a specific heat of metal?

Specific heat is amount of energy, measured in either joules or calories, needed to raise the temperature of one gram of the substance one degree Celsius. The metals will be heated to a high temperature then placed into the calorimeter containing a known quantity of water at a lower temperature.

How do you calculate the specific heat of a metal?

Q = m*s*dT, where Q = heat, m = mass, s = specific heat, and dT is the change in temperature (T2 – T1). You can use this formula to calculate the specific heat.

How do you solve for the final temperature?

Add the change in temperature to your substance’s original temperature to find its final heat. For example, if your water was initially at 24 degrees Celsius, its final temperature would be: 24 + 6, or 30 degrees Celsius.

What is the specific heat of water and metal?

These problems are exactly like mixing two amounts of water, with one small exception: the specific heat values on the two sides of the equation will be different. The water specific heat will remain at 4.184, but the value for the metal will be different. These values are tabulated and lists of selected values are in most textbooks.

What happens when you mix metal with cold water?

a) The colder water will warm up (heat energy “flows” in to it). The warmer metal will cool down (heat energy “flows” out of it). b) The whole mixture will wind up at the SAMEtemperature. This is very, very important.

What is the final temperature (in °C) of the iron block?

If the heat released during condensation goes only to warming the iron block, what is the final temperature (in °C) of the iron block? In order to continue the calculation, you need to know the specific heat of iron. This source says 0.444 J/g °C. 24.0 °C + 55.6 °C = 79.6 °C

What happens when a piece of iron is placed in water?

Example #1:Determine the final temperature when a 25.0 g piece of iron at 85.0 °C is placed into 75.0 grams of water at 20.0 °C. First some discussion, then the solution. Forgive me if the points seem obvious: a) The colder water will warm up (heat energy “flows” in to it). The warmer metal will cool down (heat energy “flows” out of it).