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Ethanol (molar mass = 46 g/mol) can be dehydrated to yield ethene (molar mass = 28 g/mol) by heating it with an excess of concentrated sulfuric acid (acting as a catalyst). CH3CH2OH CH2=CH2 + H2O If 23.3 g of ethanol produced 12.5 g of ethene, the percentage yield of the product equals
What is the final temperature of the sand A 1.00 kg gold bar at 1010 K is dropped into 0.750 kg of sand at twenty five degree Celsius?
How much heat is released by 100.0 mL of a dilute solution of NH4NO3 as it changes its temperature from 22.4C to 19.1C when it is being prepared?
Write the net ionic equations for & the reactions occurring for each cation in the group.
How many grams of potassium hydroxide (KOH) must be dissolved in 820 mL of water to make a solution with a pH = 11.1?
2.00 x10^2 mL of .744 M HCl is mixed with 2.00 x 10^2 mL of .372 M Ba(OH)2. how many moles of water are produced in the reaction
For the cell as written, what is the voltage after the addition of the following volume of NaI solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction
How many grams of sucrose must be added to 552 g of wwater to give a soution with a vapor pressure 2.0 mm Hg less than that of pure water at 200C ?( the vapor pressure of water at 200C is 17.5 mm Hg)
Three manufacturers are producing carbonated bottled water. One company introduces carbonate by bubbling carbon dioxide into water until
The Ka for cacodylic acid (C2H7AsO2) is 5.37 x 10-7. An amount (0.1035 g) of this compound is added to 0.5 L H2O. What is the resulting pH of this solution
When steam (hot water) is passed over iron, hydrogen gas and iron (3) oxide are formed. What weight of steam would be needed to react completely with 100.0g of iron.
How much energy in kilojoules is required to convert 260 mL of water at its boiling point from liquid to vapor?
Ferrophosphorus reacts with pryite producing iron(II) sulfide and a compound that is 27.82% P and 72.13% S by mass and has a molar mass of 444.56 g/mol. a) determine the empirical and molecular formulas of this compound. b) Write a balanced chemic..
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