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You have a 1.00-mole sample water at and you heat it until you have gaseous water at . What is the q for the entire process? Use the following data.

 

Specific heat capacity of ice:  

Specific heat capacity of water:  

Specific heat capacity of steam:  

 

   

   

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Matt Ocampo
Matt OcampoLv10
9 Nov 2020

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Related questions


5.00 g sample of aluminium pellets (specific heat capacity 0.89 J oC-1 g-1) and a 10.00 g sample of iron pellets (specific heat capacity 0.45 J oC-1 g-1) are heated to 100.0 oC. The mixture of hot iron and aluminium is dropped into a beaker containing 100 g of water at 15 oC. What is the final temperature of the liquid water? Heat capacity of liquid water is 4.18 J oC-1g-1; of ice 2.05 J oC-1 g-1; of steam 1.996 J oC-1 g-1; ?Hvap 40.7 kJ mol-1; ?Hfusion = 6.0kJ mol-1

Determine

how much

energy in kJ would be transferred if 300.0 grams

of steam (gaseous

water) at 150.0

̊C

is cooled to ice

(solid water)

at -20.0

̊C.

The specific

heat

of steam is

1.86

J/(g∙ ̊C),

the

specific heat

of ice is 2.06

J/(g∙ ̊C),

the heat of fusion of water

is 333

J/g, and

the heat

of vaporization is 2256 J/g.

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