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For an addition polymerization, the initiation is the slow step (1st order in initiator,R'2------->2R'.). The propagation step is fast with the rate=k1[R.][monomer]. The termination step is also fast with rate=k2[R.]^2. Explain why low concentrations of initiator are used to achieve long polymer chains.
Compute the equilibrium concentration of La3+ in the resulting solution. Ignore activity coefficients. Ksp = 1.0 x 10-11 use the below equation to find the net ionic equation. KIO3(aq) + La(NO3)3(aq) ---> La(IO3)3(s) + KNO3(aq)
A solution is prepared by dissolving 297 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.)
Calculate What will be the volume of this gas sample at standard atmospheric pressure and
Propose a mechanism for the following reaction, using arrows to show the flow of electrons. Be sure to show every step.
Explain why the elimination reaction in acetone promotes an E2 mechanism while water promotes and E1 mechanism? Which product is more thermodynamically stable, the E or Z isomer?
What would be your average speed in cm/s?(c) what would be your time (in minutes:seconds) for 1500m? show your work
What is the number of moles of O2 needed to burn 260.0g of C2H2 in the reaction: 2C2H2 + 5O2 yields 4CO2 + 2H2O?
The empirical formula is NO2. If the molar mass is 92g/mol give the molecular formula.
Add charges, single electron dots, and/or pairs of dots as appropriate to show the Lewis symbols for the most stable ion of each element. Treat as the valence shell in all cases. To add formal charges, click the button below (which will turn yello..
Celsius and heated to the temperature of 275 degree Celsius at a constant pressure of 0.975 atm. compute the work done?
Determine the mass of the hydrate and the mass of the sulfate after removing the water. 2. Calculate the number of moles of water and the number of the moles of the anhydrous sulfate
suppose 7.70g of methane is mixed with 54.7g of oxygen . Calculate the maximum mass of water that could be produced by the chemical reaction
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