Acup holding 125.12g of water has an initial temperature of 26.8 degrees c. after a 35.08g piece of metal, at 99.5 degrees c, is transferred to the water, the temperature rises to 29.7 degrees c. what is the specific heat of the metal?

0.620 J/g°C

Heat gained or absorbed, Q by a substance is calculated by;

Q = mass × specific heat capacity × Change in temperature

In this case we are given;

We are required to calculate the specific heat capacity of the metal;

Specific heat capacity of water = 4.184 J/g°C

Temperature change of water = 29.7 °C - 26.8°C

                                                   = 2.9 °C

But, Q = m×c×ΔT

Thus, Heat = 125.12 g × 2.9°C × 4.184 J/g°C

                  = 1518.156 Joules

Specific heat capacity of the metal = x J/g°C

Temperature change of the metal = 29.7 °C - 99.5°C

                                                         = -69.8 °C

But, Q = mcΔT

Therefore;

Heat lost by the meatl = 35.08 g × x J/g°C × 69.8 °C

                                     = 2.448.584x Joules

The heat gained by water is equal to the heat lost by the metal

Therefore;

1518.156 Joules = 2.448.584x Joules

x = 1518.156 J ÷ 2.448.584 J

   = 0.620 J/g°C

Therefore, the specific heat of the metal is 0.620 J/g°C

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.