The heat of fusion AH, of methanol (CH,OH) is 3.16 kJ/mol. Calculate the change in entropy AS when 23. g of methanol melts at -98.0 °C. Be sure your answer contains a unit symbol. Round your answer to 2 significant digits. 0 0 ロ･ロ X H Olo

In the following experiment, solid CaCl2 (M = 110.98 g/mol) is dissolved in water:CaCl2(s) → Ca2+(aq) + 2Cl-(aq)     ΔsolnH = ? kJ mol−1A 4.00 g sample of CaCl2 is added to a coffee-cup calorimeter containing 125 g of H2O. The initial temperature of water in the calorimeter is 22.0°C and the final temperature is 27.5°C. What is the enthalpy change for the dissolution reaction (ΔsolnH) in kJ per mole of CaCl2? Assume the specific heat capacity of the solution is the same as water (Cs=4.18 J g-1 °C-1) and that no heat is lost to the calorimeter.

3 If we measure the heat change (q) of everything in a system except the calorimeter, we can use the first law of thermodynamics (∆Euniverse = 0) to calculate the heat change of the calorimeter (qcal).  In this reaction, we combine 5.75 g of 67.4 ºC water with 6.67 g of 19 ºC water in a calorimeter.  Since some of the heat is absorbed by the calorimeter, the final temperature of the water is 25.4ºC.  Since the hot and cold water are combined, the final temp of the water is the final temp for the hot water and the cold water.  Calculate the heat change of the calorimeter in J. Remember that all of the heat changes must add up to zero so you can calculate the heat change of the hot water (qhotwater) and the heat change of the cold water (qcoldwater) using for each where Cs = 4.186 J/gºC.  The first law of thermodynamics tells us that all of these changes sum up to zero so   Enter your answer to one decimal place (tenths)

Find the ΔH (in kilojoules) for the reaction below, given the following reactions and subsequent ΔH values: (Write your answer in 1 decimal place without the unit). N2(g) +  2O2(g)  →  2NO 2(g) N2(g)  +  3H2(g)  →  2NH3(g)                                  ΔH = -115 kJ 2NH3(g)  +  4H2O(l)  →  2NO2(g)  +  7H2(g)          ΔH = -142.5 kJ H2O(l)  →  H2(g)  +  1/2O 2(g)                                 ΔH = -43.7 kJ