QUIZ 8 1. When 25.0g of HO at 804C is added to 100 g HO at 24.7C in a calorimete
ID: 1043293 • Letter: Q
Question
QUIZ 8 1. When 25.0g of HO at 804C is added to 100 g HO at 24.7C in a calorimeter (also at 24.7C ne equilibrium temperature is 35.O'c.(10 points) a. How much heat is lost to the b. Calculate the heat Ii/C) of the calorimeter 2. The lactice energy (endothermic process) for most salts exceeds the hydration energY (exothermic a is the dissolving process for most salts an endothermic or exothermic process? b. Does the solubility of most salts increase or decrease with temperature 3. A 3444g sample of an unknown metal, heated to 98.6C, is transferred to 50.0 mL of The equilibrium temperature is 28.3'C 0 H,0 at 22.2°C, What is the specific heat of the metal? (Explanation / Answer
I am solving the Q1 as per Chegg guidelines, post multiple question to get the remaining answers
Q1)
a) Heat lost by water at 80.4C = mass * specific heat capacity * change in temperature
=> 25g * 4.184 J/gC * (80.4 - 35)
=> 4748.84J
Heat gained by water at 35C = mass * specific heat capacity * change in temperature
=> 100g * 4.184 J/gC * (35-24.7)
=> 4309.52J
Heat lost to the calorimeter = 4748.84 - 4309.52 = 439.32J
b)
Heat capacity of the calorimeter = Heat lost/change in temperature
=> 439.32/(35-24.7)
=> 42.652 J/C