Question

can someone help me with these and explain calculations

process 1) Dissolving process for most salts an a) Exothermic b) Endothermic with temperature increase. 2) The solubility of most salts ( a) Decrease b) Increase c) Unaffected 3) The molar AHn (enthalpy of neutralization of a strong acid and a strong base is constant within experimental error. Is it true or false? a) True b) False 4) When 25.0 g of H20 at 80.4°C is added to 100 H2O at 24.7°C in a calorimeter (also at 24.7°C), the equilibrium temperature is 35.0°C. a. How much heat is lost to the calorimeter? a) 235J b) 439J c) 36J d) 556J 5) A 34.44-g sample of an unknown metal, heated to 98.6°C, is transferred to 50.0 mL of H2O at 22.2°C. The equilibrium temperature is 28.3°C. What is the specific heat of the metal? (specific heat of water is 4.18 J/g °C) 9=SMAT a) 0.527 J/g•°C b) 1.054 J/g•°C c) 0.845 J/g•°C d) 5.274 J/g•°C

Answer 1

(I.) Dissoluing process for most salts is an endothermic a флосед. Explanation. The dissoluing process is a physical process not a Chemical reaction. The ions are inuolued in structuring the solid and goes in specific patterns to form crystals. The bonding energy associated in making such crystals are called lattice energy and when the solid crystal dissolued in water this lattice energy is required to tranform 2. Ultimately the energy is collected a from enuironment (which is water) to let its temperature dropped: