In the laboratory a \"coffee cup\" calorimeter , or constant pressure calorimete

Question

In the laboratory a "coffee cup" calorimeter, or constant pressure calorimeter, is frequently used to determine the specific heat of a solid, or to measure the energy of a solution phase reaction.

Since the cup itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter and the value determined is called the calorimeter constant.

One way to do this is to use a common metal of known heat capacity. In the laboratory a student heats 98.15 grams of nickel to 98.47 °C and then drops it into a cup containing 80.82grams of water at 24.52 °C. She measures the final temperature to be 32.92 °C.

Using the accepted value for the specific heat of nickel , calculate the calorimeter constant. Calorimeter Constant =  J/°C.

Explanation / Answer

specific heat of nickel = 0.44 J/goC
specific heat of water = 4.18 J/goC

Initial temperature of water and calorimeter was same
Let Calorimeter constant be C J/oC

use:
Heat lost by nickel = heat gained by water and calorimeter
m(Ni)*C(Ni)* deltaT (Ni) = m(water)*C(water)* deltaT (water) + C* deltaT (Calorimeter)
98.15 * 0.44 * (98.47 - 32.92) = 80.82 * 4.18*(32.92 - 24.52) + C *(32.92 - 24.52)
2830.84 = 2837.75 + C *8.4

C is coming as negative

Your data is wrong somewhere

My process is correct
Please put the correct values and you will get the answer

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