The 116-g sample was heated to 94.5°C and placed into a calorimeter containing 72 g of water at 20.0°C. The heat capacity of the calorimeter was 14.7 J/K. The final temperature in the calorimeter was 25.6°C. What is the specific heat capacity (in J/g°C) of the mineral?

0.2212 J/g.k

Explanation:

The law of conservation of Energy states that the sum of heat given out by the mineral in the system and the heat absorbed by the water and calorimeter are equal to zero.

This implies that:

We can as well say that:

             ----------------equation (1)

Also, heat absorbed by the calorimeter which is denoted by;

              ---------------- equation (2)

where;

= heat capacity of the calorimeter

= change in  temperature

However, the heat released by the mineral and the one absorbed by the water in the system is given as:

Q = mcΔT                       ------------------  equation (3)

where;

m = mass

c = specific heat capacity

ΔT = change in temperature

If we substitute the two prior equation (i.e equation 2 and 3) into equation 1: we have;

            ---------------- equation (4)

Now , let's state our given parameters;

Given that:

mass of water () = 72g

The specific Heat capacity of water () = 4.18 J/g.k

change in temperature () =25.6 °C - 20°C

change in temperature () = 5.6 °C                  

(since we are asked to leave our answer in J/g°C)

Heat capacity of calorimeter = 14.7 J/k

change in temperature () =  5.6 °C

mass of the mineral = 116 g

change in temperature of the mineral () = 25.6 °C - 94.5 °C

change in temperature of the mineral () = -68.9 °C

specific heat capacity  of the mineral

∴ substituting all our values into equation (4); we have:

= 0.221172 J/g°C

= 0.2212 J/g°C

let that person have a turn to speak : )

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error