[sassychar]

I need help on 3 questions..


1)  In a caliorimeter, 100.00 mL of 1.0 M NaOH and 100.00 mL of 1.0 M HCl are mixed . Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0g/cm^3 and a specific heat capacity of 4.18 J/degrees Gram, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.


2) In a calorimeter, 50,0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed to yield the following reaction:

Ag+(aq) + Cl-(aq)----> AgCl (s)

The two solutions were initially at 22.6C and the final temperature is 23.4C. Calculate the heat that accompanies this reaction. Assume that the combined solution has a mass of 100.0g and a specific heat capacity of 4.18J/degrees C Gram. Calculate the Delta H for the reaction in kJ/mol.

3) use the data to determine the heat of combusion of a candle made of paraffin:

Mass of water in calorimeter: 340 g
Temperature of Water at Start: 15.0C
Temperature of Water at End: 31.2C
Mass of candle at start: 24.7g
Mass of candle at end: 23.6g


THANKS THANKS and happy thanksgiving!

[Yggdrasil]

Please read the Forum Rules.  You should that you've at least attempted to answer the problem before we will help you.

Hint: the formula you should be using is q = mCΔT