Ans 22 B. 0.65%
Let us assume the mass of pepsi can be 100 g
so sugar in it would be 11 g
and water will be 89 g
number of moles of sugar will be 11 / 342.3 = 0.0321 moles
number of moles of water will be 89 / 18 = 4.944 moles
total number of moles = 0.0321 + 4.944 = 4.976
Mole percent of sugar = (0.0321 / 4.976) x 100
Mole percent of sugar in soda = 0.65%
A can of Pepsi is about 11% by mass sugar (C _12 H_22 O_11 ; molar...
What is the mole fraction sucrose when 295 g sucrose C 12H 22O 11 (molar mass 342.3 g/mol) is dissolved in 405 g water?
The density of a 0.84 M aqueous sugar (C12H22O11) solution is 1.12 g/mL at 25°C. What is the molal concentration? The molar mass of C12H22O11 = 342.3 g/mol.
What is the boiling point of a solution produced by adding 650 g of cane sugar (molar mass 342.3 g/mol) to 1.7 kg of water? For each mole of nonvolatile solute, the boiling point of 1 kg of water is raised 0.51 ∘C.
Sugar is easily soluble in water and has a molar mass of 342.30 g/mol. What is the molar concentration of a 245.6 mL aqueous solution prepared with 78.3 g of sugar? Suppose you have 350.0 mL of a 0.450 M sodium hydroxide solution. How many moles of sodium hydroxide are in the solution? Calculate the percent by mass of a solution made from 17 g NaCl (the solute) and 67 g water. Suppose you need to prepare 141.5 mL of...
The density of a 0.84 M aqueous sugar (C12H22O11) solution is 1.12 g/mL at 25°C. What is the molality? The molar mass of C12H22O11 = 342.3 g/mol. Dinitrogen tetroxide decomposes to produce nitrogen dioxide: N2O4 (g) ↔ 2 NO2 (g) Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100°C: [N2O4] = 0.800 M and [NO2] = 0.400 M
3.) Quinine (C,H,N,0) (Molar Mass = 324.42 g/mol) is an anti-malaria drug. An aqueous solution was mixed containing 88.8 mg (milligrams) of quinine and 1.5 liters of H.O. (assume a total volume of 1.5 L of the solution) (Density of H,0 = 1.01 g/mL) Given this data calculate the following: (Show ALL Work) a.) Mole Fraction of Quinine in Water: (5 pts) b.) The molality of quinine: (again 1.5 L of solution / solvent) (5 pts) c.) ppm of quinine:...
Ester= Isoamyl acetate (banana) Molar mass of banana= 130.19 density= 0.876 g/ml 5.26 g ester product. Alcohol= isoamyl alcohol density= 0.81 g/ml Molar mass= 88.148 g/mol Quantity= 5.4 ml Carboxylic acid= acetic acid density= 1.05 g/ml Molar mass= 60.052 g/mol Quantity= 11.4 ml and 1 ml of concentrated H2SO4 (1.8 g, 0.018 mole) was also used in the procedure. Calculate theoretical yield and % yield .
don't worry about trial 2. thank you. C. Heat of Solution of NH.NO Name Trial 2 (if necessary) Trial 20.00 mL Water volume, 1* addition Water volume, 20 addition 20.00 mL 4.184 J/g °C Total volume of water added Mass of water Assume density is 1.00 g/mL Specific Heat of water Mass of NH.NO, Molar mass of NHNO; Moles of NH.NO, 0.7479 g Initial temperature of water 23.15°C Final temperature of water 21.85 °C ΔΤ Calculate the heat absorbed or...
A calorimeter contains 29.0 mL of water at 14.0 ∘C . When 1.30 g of X (a substance with a molar mass of 61.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 27.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
An aqueous CaCl2 solution has a vapor pressure of 80.2 mmHg at 50 ∘C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? A hypothetical solution forms between a solid and a liquid. The values of the thermodynamic quantities involved in the process are shown in the following table. Action Enthalpy separation of solute 11.5 kJ/mol separation of solvent 21.8 kJ/mol formation of solute-solvent interactions -86.7 kJ/mol solute...