31. 17.1 g of calcium chloride is dissolved in 750. mL of a water (d =...
specific heat capacity 2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 25.8 °C, final temperature after dissolving is 29.9 °C. Calculate the enthalpy of solution in Joules. You may assume a density of 1.00 g/mL for the solution and you may assume that the specific heat is that of water (this is a dilute solution) and is 4.18 J/(gx°C). Is this an endothermic or exothermic...
3. When 15.7 g of calcium chloride (CaClz) was dissolved in 200.0 ml of water in a coffee-cup calorimeter, the temperature of the solution increased from 25.00 °C to 34.13 °C, the dissolution of CaCl in water in units of kJ per mole of CaCl,. Calculate the entha lpy change(AH otn)for You can assume that the calorimeter loses only a negligible quantity of heat, that the total solution is 200.0 mL (adding the solid CaCl, did not change the volume...
Calculate the freezing point of a solution of 40.0 g of calcium chloride (molar mass = 110.98 g/mol), dissolved in 800. g of benzene, C6H6. Kf for benzene is 5.10oC/m and the freezing point is 5.50oC for benzene.
how many grams of sodium chloride would need to be dissolved to make 750 mL of a 1.7 M solution?
35 g of Na2CO3 is dissolved in 150 mL of water to produce a solution with a total volume of 157.2 mL. If the water is at 33∘C, what would be the freezing point of this solution (in ∘C)
0.2650 g of a compound of unknown molecular mass were dissolved in 18.00 mL of a non-ionizing solvent with specific gravity of 0.7480. The pure solvent was determined to have a freezing point of 6.80°C. The freezing point of the solution was determined graphically. Trial one yielded a freezing point of 5.31°C for the solution. Trial two indicated the freezing point to be 5.23°C. Kf (solvent) = 12.8 C°/m a. Calculate the molecular mass of the unknown. b. If 5.50...
When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)
A solution contains 10.35 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -3.26 ∘C. The mass percent composition of the compound is 60.98% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?
A solution contains 11.70 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume a density of 1.00 g/mL for water.) The freezing point of the solution is -7.01 ∘C. The mass percent composition of the compound is 38.70% C, 9.74% H, and the rest is O. What is the molecular formula of the compound? Express your answer as a molecular formula So far I got CH3O as my empirical, but I can't seem to figure out how...
A 0.5187-gram sample of calcium chloride (CaCl2;MW 110.98g/mol) was dissolved in 300. mL of water. What is the molality of the solution? (Assume the density of water is 1.00g/ml)