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The reaction scheme goes as follows: H2PtCl6 CH3--(CH2)5--CH==CH2 <-----------------> CH3--(CH2)2--CH2--CH3 1-Octene NaBH4 Octane Ethanol 6M HCl (diluted) Givens: 120µL = 0.12mL of 1-Octene 50µL = 0.050mL of H2PtCl6 1mL of Ethanol 125µL = 0.125mL of NaBH4 100µL = 0.100mL of diluted 6M HCl -------------------- My attempt: I know that we have to convert what we have to moles (using mmols) 0.12mL of 1-Octene (using the density=0.72g/mL) = 0.76 mmol 50µL H2PtCl6 = 0.234 mmol 1mL Ethanol = 17.1 mmol 125µL NaBH4 = 3.54 mmol we can ignore the HCl because it's diluted, right? (also since we don't know the % of actual HCl dilution, so we can't use the molarity to get moles) Since we are going from 1-Octene to Octane, we have gained an extra H+ and lost a double bond. So essentially, the H2PtCl6 catalyst must have given off a H+ (since Pt metal targets alkenes). My dilemma is that I'm unsure on how to find the actual limiting reactant, and what information I should use. There's too much given; but from my introspection, we only need 1-Octene and the Pt catalyst,
Calculate the pH of a solution containing 25.00 mL of 0.12M formic acid (Ka=1.7x10^-4) to which the following amounts of 0.10M NaOH have been added:
suppose the condenser operates as a total condenser at 40 degrees, the production rate of the overhead product is 75kmol/h. The ratio of reflux and overhead product is 1.5:1.
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To 333 milliliters of a 0.120 molar Pb(NO3)2 solution, 0.667 milliliteres of 0.435 molar KIO3 is added. Calculate the concentrations of Pb+2 and IO3- in the solution at equilibrium.
a sample of a compound containing only magnesium and oxygen is found to have 194g Mg and 256g of O. What percentages of Mg and O in this compound?
A 5.0×101 sample of water absorbs 355 of heat.If the water was initially at 25.9, what is its final temperature.
A solution is prepared by dissolving 270 g of sucrose (C12H22O11) in 624 g of water. What is the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at 30°C.)
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Molecular and ionic equations, What would be the proper balanced molecular and net ionic equations for each of these neutralization reactions?
Suppose a 5.00 L sample of O2 at a given temperature and pressure contains 2.73 × 1023 molecules. How many molecules would be contained in 5.00 L H2 at the same temperature and pressure.
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