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Which is more soluble in water? Briefly explain why. Acetic Acid: CH3CO(OH) OR Ethanol : CH3CH2OH I think its acetic acid because when observing its structure it is more polar than ethanol. And when using the like dissolves like rule, a more polar molecule
Hydrogren, a possible future fuel, can also be obtained from other compounds such as ethanol. Ethanol can be made from the fermentation of crops, such as corn. How much hydrogen in grams can be obtained from 1.0 kg of ethanol (C2H5OH)?
The density of a 60% (m/m) ethanol solution 0.8937g/ml , calculate the molarity of the solution , step by step . Molar mass of ethanol = 46.07
A solution of ethanol water is prepared by dissolving 10ml ofethanol density 0.789g/mol in a 100ml of a solution with density 0.982g/mol.what is the cerntration of ethanol in the solution expressed in mass percent?;mass/volume percent?
A solution consisting of water and ethanol is found to have a refractive index of 1.3541 at 20 degrees C. The refractive indices at 20 degrees C of water and ethanol are 1.3330 and 1.3610, respectively. Determine the molar composition (in percent) of the
The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.
Assume you can heat water with perfect insulation (all the heat from combustion of ethanol is transferred to water). What is the volume of ethanol required to heat 100 mL of water by 10 degrees C? (You will need to look up density of ethanol, specific heat
A solution is made by mixing 42.0 mL of ethanol, C2H6O, and 58.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 C in torr? Values at 20C ethanol density: 0.789 g/mL & vapor pressure (torr): 43.9 torr water: denisty:
A solution is made by mixing 30.0 mL of ethanol, C2H6O, and 70.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? I got an answer of 15.45 torr and it marked me incorrect and said "Your answer is the the partial
Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -125 °C to liquid
The vapor pressures of ethanol (C2H5OH) and 1-propanol (C3H7OH) are 100 mmHg and 37.6 mmHg, respectively. Assume ideal behavior and calculate the partial pressures of ethanol and 1-propanol at 35 degrees Celsius over a solution of ethanol in 1-propanol, in
A solution is made by mixing 37.0 mL of ethanol, C2H6O, and 63.0 mL of water.? Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? ethanol: 0.789 g/mL 43.9 torr water : 0.998 g/mL 17.5 torr
