Apiece of metal weighing 59.047 g was heated to 100.0 °c and then put it into 100.0 ml of water (initially at 23.7 °c). the metal and water had final temp of 27.8 °c. what is the specific heat of the metal?

The specific heat of metal is 0.403J/g°C

Explanation:

To calculate the mass of water, we use the equation:

Density of water = 1 g/mL

Volume of water = 100.0 mL

Putting values in above equation, we get:

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

The equation used to calculate heat released or absorbed follows:

      ......(1)

where,

q = heat absorbed or released

= mass of metal = 59.047 g

= mass of water = 100 g

= final temperature = 27.8°C

= initial temperature of lead = 100°C

= initial temperature of water = 23.7°C

= specific heat of lead = ?

= specific heat of water= 4.186 J/g°C

Putting values in equation 1, we get:

Hence, the specific heat of metal is 0.403J/g°C

1 is the answer to this problem

answer: atomic mass was originally used to arrange elements on the periodic table, but is no longer used to organize the modern version.

explanation:

originally atomic mass was used to arrange elements on the periodic table from left to right in a row. each column then shows similar properties of elements of a group.

in modern periodic table, the atoms are arranged in increasing atomic number. as atomic number represents the number of protons in an atom which is unique for every atom.