g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Using the A 235.0 g sample of metal is heated to 100.0°C and poured into a calorimeter containing 50.0 specific heat of water, 4.18 J/g°C, determine the specific heat of the metal from equalion Use equation 5 needed. 25mo1°c MM= Specific heat

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The second picture is eq 5 which is needed to solve. Not another question just in case it gets flagged 

Use equation 5 to find the approximate molar mass of the metal. Show your work! Use back if
specific heat of water, 4.18 J/g°C, determine the specific heat of the metal from equation 3.
g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Using the
A 235.0 g sample of metal is heated to 100.0°C and poured into a calorimeter containing 50.0
g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Osn 3
needed. a5 mo1°c
MM-
Specific heat goC
Transcribed Image Text:Use equation 5 to find the approximate molar mass of the metal. Show your work! Use back if specific heat of water, 4.18 J/g°C, determine the specific heat of the metal from equation 3. g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Using the A 235.0 g sample of metal is heated to 100.0°C and poured into a calorimeter containing 50.0 g of water at 20.5°C. The equilibrium temperature of the water and metal is 30.5°C. Osn 3 needed. a5 mo1°c MM- Specific heat goC
MM
25
mol °C
having units ofg/mol
(equation 5)
%3D
specific heat in
g °C
Transcribed Image Text:MM 25 mol °C having units ofg/mol (equation 5) %3D specific heat in g °C
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