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23 Nov 2019

50.0 mL of deionized water at 82.3 degrees Celcius are added toa calorimeter containing 50.0 mL of deionized water at 21.1 degreesCelcius. The final temperature of the water is 50.0 degreesCelcius. Use the following values for density and specific heat ofwater, respectively: 1.00 g/mL and 4.184 J/g degrees Celcius.

1) calculate the number of Joules released by the hot water.

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Jamar Ferry
Jamar FerryLv2
29 Jun 2019

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Related questions

A 51.5g metal that had been submerged in boiling water was quickly transferred into 64.5 mL of water initially at 21.90 degrees Celcius. The final temperature is 29.20 degrees Celcius. The specific heat of water is 4.184 J/g(deg.Celcius), the experiment was performed under normal atmospheric pressure, and assume the density of water is exactly 1 g/mL. Using this information what is the specific heat of the metal in J/g(deg.Celcius)?

the ?H per mole of CaCl=-81.0kJ. Calculate the final temperature ofan aqueous solution if 30g of CaCl2 is added to 100 mL of water at23 degrees celcius. Assume that the specific heat of the solutionis the same as that of water= 4.184 J*g/celcius

A 100.0mL solution of 1.05 H2SO4 at 23.2degrees Celcius is mixed with 100.0mL of 2.0 M NaOH, also at 23.2degrees Celcius, in a coffee-cup calorimeter. After the reactionoccurs, the temperature of the resulting mixture is 35.7 degreesCelcius. The density of the final solution is 1.06g/mL. Calculatethe molar heat of neutralization. Assume the specific heat of thesolution is 4.184 J/g*C. The heat capacity of the calorimeter is32.5 J/C.

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