If 50.0 g of water at 15.0°C is added to 40.0 g of water at 85.0°C, what is the final temperature of the system?

When the Cacl2(s) is added to water, the following reaction occurs. Cacl (s) – Ca²"(aq) + 2CI"(aq) AH = - 81.5 kJ A 24.1 g sample of Caclz is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature (in °C) of the solution assuming no heat is lost to the surroundings, the final solution, containing Cacl2 and water, has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °c-lg-1. The molar mass of CaCl2 = 110.98 g/mol Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to one (1) decimal place. Answer: 59.0 The correct answer is: 67.3

A student followed the procedure in this experiment, using 29.5 mL of 1.59 molar HCl and 31.0 mL of 1.59 molar NaOH, with both solutions having an initial temperature of 22.6 oC.  After mixing, a maximum temperature of 33.1 oC is measured. The final mass of the mixture was found to be 64.655 grams.  For this problem, assume the  specific heat of the solution is 4.18 J/g oC. What is the heat transferred by this reaction, in Joules? Give your answer in in decimal format. When entering units, use proper abbreviated units with proper capitalization.

NW113AACE04-21 3. a hunk of metal-like substance was found in an archeological site. In an attempt to identify it, the metal was heated and placed in a calorimeter containing water and determined the specific heat of the metal. If the specific heat of the metal is 0.448 J/g °C, what is the approximate molar mass (atomic mass) and likely identity of the metal? (Hint: compare the molar mass (atomic mass) of metal that of metals in periodic table)