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why does heating dicyclopentadiene form cyclopentadiene, whereas allowing cyclopentadiene to stand at room temperature lead to dicyclopentadiene? consider, free energy, enthalpy and entropy changes in your answer
Calculate How many grams of pure, solid sodium hydroxide are needed to make 500 mL of 0.15M NaOH solution and also express the answer in just 2 significant figures?
n2 is .070 moles o2 is 0.35 moles and co2 is 0.20 moles the total is pressure 1.55 atm what is the pressure of
calculate the chloride concentration in mEq/L of a solution prepared by diluting 25 g of BaCl2 to 2 L. (WM = 208)
Using curved arrows, show how the species in part (a) can act as Lewis bases in their reactions with HCl, and how the species in part (b) can act as Lewis acids
The few gas analysis shows as carbon dioxide 14%, carbon monoxide 0.4%, oxygen 5.6% and nitrogen 80%. The air used has a dew point of 50°F. The barometer shows 29.9 inches of mercury. Calculate the dew point of the stack gas.
Draw the structural formula for 3-methylhexane and 2-butanol and identify the chiral carbon and the four "groups" attached to the chiral
How then, how would I calculate the pH of a buffer + NCl after taking 32 mL of the solution noted above and pipet 1.0 mL of 6.0 M HCl with the pH of buffer + HCl = 4.41
Calculate the molar Gibbs free energy change for the phosporylation of glucose by ATP to produce glucose-6-phosphate. Assuming the reaction happens at 310K and at pH 7. The concentration of ATP, ADP, G6P, and Glu are 1850 µM, 138 µM, 83 µM, and 50..
Introduced into a 1.70 L flask is 0.120 mol of PCl5 ; the flask is held at a temperature of 227 C until equilibrium is established. PCl5(g) PCl3(g) + Cl2(g) What is the total pressure of the gases in the flask at this point
The vapor pressure of pure CH2Cl2 (with molecular weight 85 g/mol) is 133 torr at 0?C and the vapor pressure of pure CH2Br2 (with molecular weight 174 g/mol) is 11 torr at the same temperature.
an unknown concentration and you have five samples with known concentration of the compound. List 3 pieces of information you need to determine in order to calculate the unknown concentration spectrophotometrically.
E was found to be -2,000.00 kJ/mol of an unknown liquid hydrocarbon at 298 K. In another experiment it was determined that for each mole of hydrocarbon, 5 moles of oxygen gas are consumed
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