A sample of ethanol, C2H6O, has a mass of 26.50g. Calculate the number of ethanol molecules...
A sample of ethanol, C2H6O, has a mass of 58.50 g. Calculate the number of ethanol molecules in the sample.
Calculate the moles of C2H6O in 5.66x1024 molecules of C2H6O. Calculate each of the following quantities in 1.50 moles H3PO4: moles of H, moles of O, atoms of P, atoms of O
A certain alcoholic beverage contains only ethanol (C2H6O) and water. When a sample of this beverage undergoes combustion, the ethanol burns but the water simply evaporates and is collected along with the water produced by combustion. a. A 9.8959 g sample of this beverage is cured for elemental analysis in excess oxygen and 2.1104 g of CO2 is collected. How many moles of ethanol, C2H6O are in this sample? b. What is the % volume of ethanol for this beverage.
Ethanol (C2H6O) is used as an additive in gasoline . Calculate the molality of an ethanol solution prepared by dissolving 78.6 g of ethanol in enough water to produce 225 g of solution . Select one: A. 11.67 m B. 7.59 m C. 349.33 m D. 0.349 m E. 0.537 m
Calculate energy in joules and calories, when 15.0g of ethanol is lost, C2H6O,cools from 60.5 to 42.0 ,Ethanol has 0.588cal/g degree Celsius and 2.46j/g degree Celsius
When 1775 J1775 J of heat energy is added to 49.9 g49.9 g of ethanol, C2H6O,C2H6O, the temperature increases by 14.5 ∘C.14.5 ∘C. Calculate the molar heat capacity of C2H6O.
A sample of hydrogen sulfide, H2S, has a mass of 98.50 g. Calculate the number of hydrogen sulfide molecules in the sample. molecules
1) Calculate the number of C atoms in 0.334 mole of C. Nc=______atoms of C 2) Calculate the number of SO2 molecules in 2.73 moles of SO2. NSO2=______ molecules of SO2 3) Calculate the moles of Fe in 2.82x1022 atoms of Fe. Nfe=_______ mole of Fe 4) Calculate the moles of C2H6O in 3.11x1024 molecules of C2H6O. nC2H6O=_______ moles of C2H6O
When 1.730×103 J of heat energy is added to 46.4 g of ethanol, C2H6O, the temperature increases by 15.2 ∘C. Calculate the molar heat capacity of C2H6O.
Consider ethanol (C2H5OH, or C2H6O) burning with air. The lower heating value (LHV) of ethanol is given as 26,700 kJ/kg. Compute the higher heating value (HHV) of ethanol in kJ/kg from the given LHV value and the enthalpy of vaporization of water (44,010 kJ/kmol).