A calorimeter is to be calibrated: 51.203 g of water at 55.2 degree C is added t
ID: 502984 • Letter: A
Question
A calorimeter is to be calibrated: 51.203 g of water at 55.2 degree C is added to a calorimeter containing 49.783 g of water at 23.5 degree C. After stirring and waiting for the system to equilibrate, the final temperature reached is 36.7 degree C. Calculate the calorimeter constant. Using the same calorimeter from question 2, calculate the amount of hear evolved when 50.00 mL of 0.400 M copper(II) sulfate solution at 23.35 degree C is mixed with 50.00 mL of 0.600 M NaOH solution at same temperature. After the reaction occurs, the final temperature of the resulting mixture is measured to be 25.23 degree C. The density of the final solution is 1.02 g/mL. Assume the specific heat of solution is the same as pure water, 4.184 J/g degree C.Explanation / Answer
A calorimeter is to be calibrated: 51.203g of water at 55.2°C is added to acalorimeter containing 49.783g of water at 23.5°C. After stirring and waiting for the system to equilibrate, the final temperature reached is 37.6°C.
Calculate th ecalorimeter constant.
msT+xT+ msT= 0
(cold H2O)(calorimeter)(hot H2O)
(51.203g)(4.18J/g°C)(-17.6°C) + x(14.1°C) + (49.783)(4.18J/g°C)(14.1°C)=0
X= Calorimeter constant= 59.063J/°C
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