5. When 50.0 mL of 1.00 M HCl is mixed with 50.0 mL of 1.00 M NaOH in a calorime
ID: 912079 • Letter: 5
Question
5. When 50.0 mL of 1.00 M HCl is mixed with 50.0 mL of 1.00 M NaOH in a calorimeter, a neutralization reaction takes place in which the temperature of the mixture increases from 25.0°C to 31.6°C. If the density of the mixture is assumed to be 1.00 g/mL and its specific heat is assumed to be 4.18 J/g.°C, how much heat (in kJ) is released by this reaction, assuming the calorimeter absorbs no heat? a. 23.6 b. 13.2 c. 6.60 d. 2.76 e. 1.38
6. A 47.5 gram sample of a metal at a temperature of 425°C is placed in 1.00 liters (1000 grams) of water which had an initial temperature of 18°C. What is the specific heat capacity of the metal if the final temperature of the metal and water at equilibrium is 21°C? (The specific heat capacity of water is 4.18 J/°C·g.) a. 0.65 J/°C·g b. 0.03 J/°C·g c. 1.47 J/°C·g d. 12.54 J/°C·g e. -0.75 J/°C·g
Explanation / Answer
5. mass of the solution = (50+50)*1 = 100 grams
s = specific heat = 4.18 j/g.c
DT = 31.6-25 = 6.6 c
q released = 100*4.18*6.6 = 2758.8 joule
= 2.76 kj
answer ; d.2.76 kj
6.
q lost by metal = q gained by water
mmetal*smetal*DT = mwater*s*DT
47.5*S*(425-21) = 1000*4.18*(21-18)
s = specific heat of metal = 0.65 j/g.c
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