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Would this reaction be an example of saponification? phenyl-COOCH2CH3 + NaOH ----> phenyl-COONa + CH3CH2OH I ruled out Aldol condensation and enolization, and I don't think it's esterification, but it doesn't quite fit the description of saponification in the text or in my head
Hydrogen Sulfide decomposes to the reaction 2H2S--->2H2+S2. Delta S= 78.1 j/k and the Delta H=169kJ. At what temperature would the reaction be spontaneous
Water in the sample extracts into the methanol, which is then analyzed. If GC analysis of the methanol yields a peak height of 13.66, what is the % w/w water in the antibotic?
exhales 30.0 times per minute, that the exhaled air is at a pressure of 1.00 atm, and that the air behaves as an ideal gas. Calculate the time in hours before a fire fighter using such an air tank runs out of air.
If it is known that 41.6 grams of PURE ELEMENT THAT IS NOT DIATOMIC represents 1.30 moles of this element, what is the atomic mass of the element?
Suppose you were given a pure stereoisomer that rotated the plane polarized light either +60 degrees or -120 degrees, i.e a uniform colour is observed for both of these readings.
What is the percent by mass of a solution in which 60. g of NaOH are dissolved in sufficient water to make 100 g of solution.
The density of benzene at 25.0 degrees C is 0.879g/cm3. What is the volume in liters of 2.5 kg benzene?
Describe the physical origins of linewidths in absorption and emission spectra. Do you expect the same contributions for species in condensed and gas phases
Calculate the molar heat of vaporization of a substance given that 0.383 mol of the substance absorbs 24.1 kJ of energy when it is vaporized.
a. A 0.1044 gram sample of an unknown monoprotic acid required 22.10 mL of 0.0500 M NaOH to reach the end point. What is the molar mass of the unknown?
Consider a situation in which 161g of P4 are exposed to 176g of O2. A)What is the maximum amount of P2O5 that can theoretically be made from 161g of P4 and excess oxygen
Calculate w (in kJ) when 376 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 335 K:
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