Question

Lab 11: Calorimetry: The Determination of the Specific Heat of a Metal directions exactly. How would the experiment POST-LABORATORY QUESTIONS 1. In doing this experiment, a student did not follow the directions exactly. How we be affected if the following were done? a. Glass beakers were used to make the calorimeter instead of Styrofoam cups. b. Not all of the water was delivered from the 50 mL volumetric pipet to the calorimeter c. No plot of temperature was carried out. Instead, the student used the value of the water just after mixing with the metal as the maximum temperature. 2. Calculate the amount of heat (in calories) absorbed when 50.0 g of water at 20° C spreads over your skin and warms to body temperature, 37°C. 3. A 102.5-g sample of metal beads was heated in a water bath to 99.5°C. The metal was then added to a sample of water (25.7 g) and the temperature of the water changed from an initial temperature of 20.0 C to a final temperature of 41.5 C. a. What was the temperature of the metal at equilibrium? b. What was the temperature change of the metal? c. Calculate the specific heat and the atomic mass of the metal What is the metal?

Answer 1

SOLN 1

(a) Glass has a lesser heat capacity (speific) compared to styrofoam. that means it requires lesser amount of energy to exchange heat compared to styrofoam. Hence glass calorimeter will have lesser calorimeter constant

so the observed value of heat exchange will be lesser than actual

(b) The value of recorded mass will be errorneous and this would lead to false results.

(c) This would lead to errorneous calculations of Specific heat as calculations mainly depends on the temperature change i.e final maximum temperature at which water will be heated

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