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Draw a Lewis structure for each of the following compounds. Specify the hybrid orbitals that overlap to form each bond. Then label each bond as a pi or sigma bond. Finally, draw all nonbonding hybrid orbitals.
a.) H3COH
b.) HCCCH2OH
c.) H3CCOCH3
The melting of ice requires 1.44 Kcal/mol. If this energy goes into breaking H-bonds, how many H-bonds will there be in liquid water at 0°C?
Estimate the molar heat of vaporization of a liquid whose vapor pressure doubles when the temperature is raised from 85 ºC to 95 ºC.
A student found that her mixture was 15% NH4Cl and 75% SiO2 .Assuming her calculation are correct, what did she most likely do incorrect in her experiment?
The enthalpy change for melting ice at 0°C and constant atmospheric pressure is 6.01 kJ/mol. Calculate the quantity of energy required to melt a moderately large iceberg with a mass of 1.39 million metric tons. (A metric ton is 1000 kg.)
Draw the molecule by placing atoms on the grid and connecting them with bonds. Do not identify the charge on each of these species. Include all lone pairs of electrons.
Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.
Why is HC2H3O2 not a good conductor or strong electrolyte?
Which best describes a solid?
Nitrogen gas has a Henry's law constant k = 6.3 × 10-4 M/atm at 25°C. The "bends" in divers results from bubbles of N2(g) being rapidly released from body fluids when a diver ascends to the surface too quickly.
Calculate the mass percent of a solution that is prepared by adding 61.4 g of rm NaOH to 413 g of {rm H_2O}.
Converting liquid H2O to solid ice releases 1.44 kcal/mol. How many k/cal are released by freezing 1.4 mol of H2O?
solution made from 6.50g of an unknown compound in 27.8g of diphenyl has a molality of .195m. Calculate the molar mass of the unknown.
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