Question

Print Name: Recitation 11 but 0.5% FCG Print Name: Print Name: Situation: 10.0 mL of 1,00 M silver(I) nitrate and 10.0 mL of 1.00 M sodium chloride aqueous solutions are thoroughly mixed in a calorimeter that has a heat capacity of 20.1/°C. A white dense precipitate is formed and settles to the bottom calorimeter (cup). The gram specific heat of the final product solution is 3.861J/g °C. The density of the final product solution is 1.10 /cm at the final temperature of the product solution. The initial observed temperature of the calorimeter and reactants was 25.0 °C and the final temperature of the product solution and calorimeter is 31.1°C, using a microthermometer. Specifically calculate the heat of formation for solid silver(I) chloride. Strategy below includes the implied tasks.... a. Print the net ionic equation for the production of the dense white precipitate. Phase, arrow, and thermicity are parts of the net ionic equation. Ag Noz + NaClos Al + No Nagar) Attichen + VON ACIS) + NO Na Label which ion is the Lewis base. Label which ion is the Lewis acid. c. Calculate the number of moles related to the precipitate assuming 100.0% conversion. c. Calculate the mass of final products. (Does the mass of the products = mass of reactants?) d. Calculate the temperature change for the products and the calorimeter. What is the sign?

Answer 1

a) The reaction that occurs is:

AgNO3 + NaCl = AgCl + NaNO

Ag + + Cl- = AgCl

b) The moles that precipitate are calculated:

n AgCl = M * V = 1 M * 0.01 L = 0.01 mol

c) The final precipitate mass is calculated:

m AgCl = n * MM = 0.01 mol * 143.32 g / mol = 1.43 g

d) The temperature change:

ΔT = 31.1 - 25 = 6.1 ° C

If you liked the answer, please rate it in a positive way, you would help me a lot, thank you.