A sample of metal weighing 35.5g at a temperature of 100 ºC was placed in a calo

Question

1. A sample of metal weighing 35.5g at a temperature of 100 ºC was placed in a calorimeter containing 50 g of water at 25.0 ºC.  At equilibrium the temperature of water and metal was 35.5 ºC.  Calculate the heat capacity of the metal. Use your value for Cp.                     
2. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 ºC to 44.2 ºC.  Assume that the specific heat of solution is 4.18 J/gºC and that the density is 1g/mL.Write a balanced equation for the above reaction.  Calculate the enthalpy of reaction per mole of magnesium. Use your value for Cp.  

1. A sample of metal weighing 35.5g at a temperature of 100 ºC was placed in a calorimeter containing 50 g of water at 25.0 ºC.  At equilibrium the temperature of water and metal was 35.5 ºC.  Calculate the heat capacity of the metal. Use your value for Cp.                     
2. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 ºC to 44.2 ºC.  Assume that the specific heat of solution is 4.18 J/gºC and that the density is 1g/mL.Write a balanced equation for the above reaction.  Calculate the enthalpy of reaction per mole of magnesium. Use your value for Cp.  

Explanation / Answer

Multiple questions. Please add the second part as a separate question.

Let the heat capacity of the metal be S.

Total heat lost by the metal = 35.5 * S * (100-35.5) = 2289.75 S

Total heat gained by water = 50 * 4.179 * (35.5-25) = 2193.975

Total heat lost = toatal heat gained

=> 2289.75 * S = 2193.975

=> S = 0.96 J/gºC ( answer )

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.