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Ethanol (C2H5OH) melts at -114 degrees Celsius and boils at 78 degrees Celsius. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. ( It also says see the periodic table with a link to it)
Important information about Chair Conformation, Circle the least stable conformation as well.
Estimate the average rate of production (Using this rate) of oxygen over the same time period. Considering the given equation 2H 2 O 2 --> 2H 2 O+O 2 -H 2 O 2
Multiple choice questions in Nuclear reactions - make nuclear fission more efficient, which device is used in a nuclear reactor to slow the speed
Identify the steric number, shape, hybridization about the central atom and molecular polarity of sulphuryl chloride, SO2Cl2.
A water skier is pulled by a net force of 135 N and has an acceleration of 1.8 m/s2. What is the mass of the skier.
Important information about Organic Chemistry, The most reasonable formula for a compound demonstrating M+ =101 with a minor M+1 peak is
Calculate the heat given off by the burning Mg in kJ/g. b)Calculate the heat given off by burning Mg in kJ/mol
A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?
Rubidium has two naturally occuring isotopes. The relative abundance of rubidium-85 is 72.17%; its atomic mass is 86.91 amu. Determine the average atomic mass of rubidium.
Calculate the values of E for the cell when the following volumes of the Ce^4+ titrant have been added. (Activity coefficients may be ignored as they tend to cancel when calculating concentrations of ratios.
A 4.63 g sample of a molecular compound is dissolved in 103 g of tetrachloromethane (carbon tetrachloride). The normal boiling point of the solution is 61.51?C.
A 250.0 ml sample of gaseous hydrogen bromide, measured at 22.9 C and 0.930 atm, was dissolved in sufficient pure water to form 250.0 ml of solution. What was the pH of that solution.
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