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Predict which of the compounds should undergo a more rapid reaction with potassium tert-butoxide. EXPLAIN your REASONING and give the product of the reaction? (a) cyclopentene with a CH2Br attached. The double bond is ortho from the CH2Br. (b) cyclopentane with a CH2Br attached In (a) and (b), I believe it is the compound + potassium tert-butoxide and this goes to what MAJOR product in each instance and why?
Determine the wavelength, of an alpha particle with a(KE) kinetic energy of 8.0 10-13 Joules
Determined if CS 2 of 2.500 grams mix with an excess of chlorine gas , 9.310 Kilo joule of heat is evolved. What sort of reaction is this , Is the reaction exotermic also find out delta H for the reaction?
The combustion of 45.0 g of methane (natural gas) releases 2498 kJ of heat energy. How much energy in kilocalories kcal would combustion of 0.670oz of methane release.
the Ideal Gas Law to calculate the pressure of the vapor at 88 °C; at 66 °C. b) Will condensation occur at 88 °C; 66 °C? Explain. c) On the basis of your answers in a) and b), predict the pressure exerted by the water vapor in the flask at 88 °C; ..
calculate the amount of heat transfered when 24.0 g of CH3OH decompose at constant pressure. delta H is 126.4 kJ
what is the volume of 45.6g of silver if the density of silver is 10.5g/ml?
A laboratory method of preparing oxygen gas involves decomposition of solid potassium chlorate. The products of the reaction are solid potassium chloride and oxygen gas.
What is the total electronic energy
when 7.50g of magnesium reacts with 9.50g hydrochloric acid, hydrogen gas is formed. what is the limiting reagent?
Determine the second order rate constant from the initial concentration and half life and what is the second order rate constant?
A mixture at equilibrium at 827 C contains .552 mol CO2, .552 mol H2, .448 mol CO, and .448 mol H20. The balanced equation is shown below: CO2(g) + H2(g) CO(g) + H2O(g) What is the value of Keq?
Calorimetry is a method used to measure enthalpy, or heat, changes that occur during chemical processes. Two common calorimeters are constant-pressure calorimeters and constant-volume (or "bomb") calorimeters
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