Which of the following processes will result in the lowest final temperature of
ID: 966599 • Letter: W
Question
Which of the following processes will result in the lowest final temperature of the metal water mixture at when thermal equilibrium is reached The specific heat capacity of cobalt is 0.421 J/(g degree C). The specific heat capacity of water is 4.184 J/(g degree C). the addition of 100 g of cobalt at 95^degree C to 80 mL of water at 25^degree C in an insulated container the addition of 100 g of cobalt at 95^degree C to 100 mL of water at 25^degree C in an insulated container the addition of 100 g of cobalt at 95^degree C to 40 mL of water at 25^degree C in an insulated container the addition of 100 g of cobalt at 95^degree C to 20 mL of water at 25^degree C in an insulated container the addition of 100 g of cobalt at 95^degree C to 60 mL of water at 25^degree C in an insulated containerExplanation / Answer
The equation for Q is
Q = specific heat capacity x mass x diffrence in temeperature
Qwater = Q metal salt
density of water is 1g/ml
a) 4.184 x 80 x T1-25 = 0.421 x 100 x 95-T1
334.7 x T1-25 = 42.1 x 95-T1
334.7T1 - 8367 = 3999.5 - 42.1T1
376.8 T1=12366.5
T1 = 32.8
b)
4.184 x 100 x T1-25 = 0.421 x 100 x 95-T1
418.4 x T1-25 = 42.1 x 95-T1
418.4T1 - 8367 = 3999.5 - 42.1T1
460.5 T1=12366.5
T1 = 26.85
Since the tempearture and mass of Cobalt is the same and since temperature of water initial is the same the quantity of water decides which will give lower temperature and the higher the water quantity the lower will be the temperature so the correct answer is
b) The addition of 100g of Co at 95 C to 100 ml water at 25C
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