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When 1 mol of glucose is burned, 2802.5 KJ of energy is released. Calculate the quantity of energy released to a person by eating 5.00g of glucose in a candy.
(6x12.01 g/mol) + (12x1.01 g/mol)+(6x16.00g/mol) = 180.18 g/mol
(5.00g)/(180.18g/mol)=0.0278mol
0.0278 mol x 2803.1 KJ/mol = 77.8KJ
Plot the normalized particle in a box wavefunctions for an electron in a box of 1210 pm for n=1-6 on the same plot. Are any patterns evident? what is the probability of finding an electron in the middle 605 pm for n=6
What is the percent purity of the calcium hydroxide if the titration requires 7.81 mL of the acid to reach the endpoint?
the reaction of a particular alcohol with a carboxylic acid is 3.83. What is the calculated yield of the ester?
One piece of copper jewelry at 108 degrees Celsius has exactly twice the mass of another piece, which is at 44 degrees Celsius. Both pieces are placed inside a calorimeter whose heat capacity is negligible. What is the final temperature inside the..
why doen't the mass number decrease? (because there is one less neutron). But the atomic number increases due. What happens to the electrons?
chemistry mixture of gases contains 0.200moleO2 o.4oomole N2 and 0.600mle H2 at 2.00 atm pressure what is the partial pressure of N2 in the mixture.
The mole fraction of oxygen molecules in dry air is 0.2095. What volume of dry air at 1.00 atm and 25°C is required for burning 1.00 L of hexane (C6H14, density = 0.660 g/mL) completely, yielding carbon dioxide and water
suppose a saturated solution of Barium Flouride contains 1.47*10^-2 M F-. What is the Ksp of the BaF2?
determine the freezing point depression, delta Tf, for the ionic solution. b. determine m effective for ionic solution. c. determine the van't Hoff factor, i, for the ionic compound.
138g of K and 448g of I react completely to form KI. What mass of KI would have been produced if 138g of potassium and 41g of iodine has been used?
Write equations for the half-reactions that occur at the anode and cathode for the electrolysis of each of the following aqueous solutions.
48.61g od maagnesium was dissolved in diluted sulfuric acid and 490g of MgSO4. 7H2O was isolated from the solution. How many percent of impurities did the metal contain?
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