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Draw the mechanism of the addition of HBr to cyclohexene. Identify each step, indicate intermediates.
A 24.7 g sample of pure iron at 61°C is dropped into 99 g of water at 25°C. What is the final temperature of the water-iron mixture?
making it an excellent choice as a standard acid. What is the concentration of a NaOH solution, if it takes 62.00 mL to neutralize a 0.0778 g sample of the acid?
How many moles of CO2 form when all of the butane is the lighter burns. How many molecules of gas form when the butane in the lighter burns completely
Write a balanced net equation for the reaction of Na2S with water. writing a net equation, and sodium ions are spectator ions.
The stack gas contains C02 at a partial pressure of 80 mm Hg and no CO,O2, methane or ethane. Calculate the mole fraction of methane in the fuel and the dew point temperature of the stack gas.
Explain the use of nuclear isotope in medical field and Write a paragraph expaining what nuclear isotope can be used for medical purpose
a solution of 75 ml of 0.2 m nh3 is titrated with 50 ml of 0.5 m hno3. what is the ph of the resulting solution when 17
Octane has a density of 0.692 g/mL at 20 degrees celsius How many grams of oxygen are required to burn 1.10 gal of octance.
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K.
what would the concentration of copper be in a solution created by combining 10ml of it with 10 ml of the 0.100M copper (II)sulfate solution?
Determine the magnesium content (in ppm) of a 100.00 mL sample of drinking water if the following data were obtained. Titrant is 0.0481 M EDTA, 12.78 mL were used when an aliquot of the sample was at pH 13.0
Using the van der Waals equation, calculate the pressure of 14.0 g of N2 in a 0.600 L container at 27.0 °C. The van der Waals constants
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