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Posted by on Tuesday, November 11, 2008 at 10:51pm.

1) A 15.0 g sample of nickel metal is heated to 100.0 C and dropped into 55.0 g of water, initially at 23.0 C. Calculate the final temperature of the nickel and the water, if the specific heat capacity of nickel is 0.444 j / g x C.

2) In a coffee-cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g of water at an initial temperature of 25.00°C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34°C. Assuming the solution has a heat capacity of 4.18 J/°C·g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.

  • Chem - , Tuesday, November 11, 2008 at 11:22pm

    1.
    [mass H2O x specific heat water x (Tfinal-
    Tinitial)] + [mass nickel x specific heat nickel x (Tfinal-Tinitial)] = 0
    Solve for Tfinal.

    2.
    How much heat was exchanged when the NH4NO3 went into solution.
    q = mass H2O x specific heat water x (Tfinal-Tinitial) = ??
    ?? will be J/1.60 g NH4NO3.
    Convert that to per mole NH4NO3 and convert that to kJ. The final answer will be kJ/mol.

  • Chem - , Wednesday, October 31, 2012 at 11:19pm

    57667

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