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A 0.65 g sample of fructose (MW = 180. g/mol) is burned in a bomb calorimeter that has a heat capacity of 2.69 kJ/oC. The temperature of the calorimeter increases by 3.80oC. Calculate the molar heat of combustion of fructose using the data from this experiment. Since this experiment is carried out under conditions of constant volume, we are measuring ?E. Your answer should be in kJ/mol and entered to 3 sig. fig.
What is the pH of a solution prepared by mixing 100 ml of 0.0500 M HCL with 300ml of 0.500 M HF? Ka(HF) = 7.1 x 10^-4
Steam at 100C is used to heat water. What is the minimum mass of steam required to melt 100g of ice at 0C and heat the resulting liquid to 100C?
When a ketone is treated with LiAlH4 followed by addition of water, what general class of product results?
At a given temperature, the equlilibruin constant for the system studied in an experiement is 1.40x10^2. Suppose 100.0 ml of 2.00 x 10^-3 M KSCN was mixed with 100.0 ml of 2.00 x 10^-3 M Fe(NO3)3
The equilibrium constant for CaCO3 dissolution in water at 25 celsius is 8.7 x 10^-9. Calculate the (G) Gibbs free energy for this process.
what is the mole fraction of each componet in solution? ethanol, methanol, water.
The Ka of butyric acid, C3H7COOH is 1.5 x 10-5. What is [C3H7COO-] in a 0.397 M solution of C3H7COOH
Determine the minimum wavelength of light necessary to overcome the work function of the following metals
what is the molarity of a solution that contains 36.0g of vitamin B1 hydrochloride (molar mass = 337g/mol) in 190mL of solution?
when 500 L of a 2.0 M solution of Pb(NO3)2 is mixed with an excess of 1.00 M solution of KI, how many grams of lead(II) iodine are formed?
Explain the structure for 4-ethyl-2,3-dimethyl-2-heptene?
Why is this only an approximation? Under what conditions can the selectivityremain temperature-independent?
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