A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator to cool. It is removed when the temperature ofthe water is 5.50 degrees Celsius. (Specific heat H2O(l)=4.184 j/gC.
a) how much heat (in KJ) does the water lose?
b) Describe how the entropy of the system changes in this process?
a). Heat Lost by Water= 29.424 kJ
b). Entropy of the system DECREASES. Because, Entropy is the measurement of randomness of a system and as temperature of water is reduced, the randomness of the system will reduce.Hence entropy reduces.
A dish containing 145 g of water at 54.0 degrees Celsius is put in a refrigerator...
A lead block with a mass of 46.5 g at a temperature of 76.98 degrees celsius was placed into a calorimeter containing 100.0 mL of water at a temperature of 20.6 degrees celsius. What is the equilibrium temperature if the specific heat of water is 4.184 J/g and the specific heat of lead is 0.158 J/gdegreeC?
It takes 11.2 kj of energy to raise the temperature of 145 g of benzene from 25 degrees Celsius to 70 degrees Celsius. What is the specific heat of benzene? Please show work I am trying to figure out how to work these problems. I will rate high. Thanks
It takes 11.2 kj of energy to raise the temperature of 145 g of benzene from 25 degrees Celsius to 70 degrees Celsius. What is the specific heat of benzene? Please show work I am trying to figure out how to work these problems. I will rate high. Thanks
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What is the final temperature when 100 g of iron at 90 degrees Celsius is placed in 400 g of water at 25 degrees Celsius? The specific heat capacity of iron 0.45 J/g*K and the specific heat capacity of water is 4.184 J/g*K
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