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2.71 g sample of sucrose, C6H12O6, (180.2 g/mol) was burned in a bomb calorimeter to form CO2 and H2O. The heat capacity of the calorimeter itself was 883 J/K and it contained 830.1 g of water (c = 4.184 J/g.K). If the temperature increased by 13.2°C, what is ?E (in kJ) for the combustion of 1 mole of sucrose? Enter your answer in exponential form, 1.23x104 = 1.23E4.
A sample of .755g of NaHCO3 was dissolved in 25mL of .960 M HCl. After heating, 6.7 mL of .601 M NaOH was needed to neutralize the excess acid that was not neautralized
Which of the following terms define(s) an acid according to the Bronsted-Lowry theory?
How many grams of .49% wt% aqueous HF are required to provide a 25% excess to react with 25 mL of .023 M Th^4+ by the reaction Th^4+ + 4F^- --> ThF4
Assuming that your salt was a hydrated form of a sulfate mso4 nh2o calculate n. What values are quoted in handbooks for common hydrates
Determine whether sodium monohydrogen phosphate (Na2HPO4) is neutral, basic, or acidic. First, what is its Ka when it acts as an acid? Second, what is its Kb when it acts as a base?
How many days would be required for a dose of Cu-64 to decay to 1.0% of its original concentration?
A sugar-water mixture contains 45.8 g of sugar and 108.5 g of water. What is the percent by mass of sugar and the percent by mass of water in the solution?
A solution of glyceraldehyde, C3H6O3, has a density of 1.15 g/mL, and a mass percentage of 28.1% glyceraldhyde at 25 deg C. (molar mass = 90.078g/mol)
A 3.575g sample of a monoprotic acid was dissolved in water. it took 22.67ml of a .1453 M NaOH solution to neutralize the acid. what is the molar mass of the acid
Using graphical techniques, calculate the equilibrium pH and the equilibrium concentrations of all the dissolved species for a 10^-3 M (NH4)2CO3 solution.
The tire is filled with dry air at sea level and a temperature of 60 F to 32 lb/aquare in.standard sea level pressure is 101325 Pa at 0 C (STP).
The initial concentrations of Pb2+ and Ag+ are 0.05M and for Cl- 1.5M. Assume all the present Pb2+ and Ag+ precipitate out of solution. Use the remaining Cl- concentration and the Ksp and Kf reactions for AgCl and AgCl2-, respectively, to determin..
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