Question

Post Laboratory Questions 1. A student places 138 g of an unknown metal at 99.9°C into 60.00 g of water at 22.2 °C. The entire system reaches a uniform temperature of 31.5 °C. Calculate the specific heat capacity of the metal. 2. If the correct specific heat of the metal in problem 1 is 0.25 J/gºC, calculate the percent crror. 3. While transferring the piece of unknown metal to the calorimeter, the student dropped the metal into the calorimeter and some water splashed out of the calorimeter. a. Why must this be avoided? b. The loss of water from the calorimeter would cause the calculated specific heat capacity to be lower or higher than expected? Explain.

subject: calorimetry

Answer 1

138 g 3-) 07, +(99-9-315) ure = 3105c & Mass of the metal = m = Temperature- qq. 9° Final temperature Mass of water =m=60g Temperature Final temperature Specific heat capacity = RA 22.2°C 31050 903 37 * Tz = (315-222 I calea / goc . Acc. to calorimetric formula 138 x C2 X 6804 60. XIX. 9'3 = 0·059 calloc 68.4×138 Specificic heat capacity of heat capacity of the metal = 0.059 calle 2 Specific heat copicity of metal calculated in 0.059x9.2 j/gc 60 x 903 (z. problem. I = 0.2478 0° 2478 = Error 0.25 0022 X100 1 error % of O• 25 = 0.88 %

Answered 1st two questions from this set of multiple questions.

In calorimetry total heat remain constant.