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When 5.00 g of fructose, C6H12O6, (FW 180.16 g/mol) is burned in a calorimeter whose heat capacity is 29.7 kJ/oK, the temperature increases by 2.635oK. Calculate the heat of combustion of fructose in kJ per mole.
A quantity of Oxygen (g is originally at 4.75 atm and 26 degree Celsius in a 5.00 Litre container is transferred into the same container determine the total pressure in the new container?
commercial concentrated aqueous ammonia is a solution of 28.0%, by mass, ammonia, NH3, (molar mass=17.0 g/mol) in water. the density pf the solution is .900g/mL.
a 10.00g sample of toothpaste contaning stannous fluoride gives0.145g precipitate of stannous phosphate.what is the percentage of snf2 in the toothpast sample.
osmium has a density of 22.6 g/cm3. what volume (in mL) would be occupied by a 21.8 g sample of osmium?
Calculate the heat energy released when 10.3 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point. Constants for Mercury at 1 atm: Heat capacity: 28.0 J/(mol*K) Melting Point: 234.32 K Enthalpy of fusion
What volume of ethylene glycol, C2H6O2, a nonelectrolyte, must be added to 15.0 L of water to produce an antifreeze solution with a freezing point of -30*C? What is the boiling point of the solution?
the combustion of how many moles of ethane would be required to heat
ampere current have to be applied to plate out 8.00 grams of copper metal from te aqueous copper(II) sulfate solution?
Enter the molecular, ionic and net ionic equation for the following reactioins. I am having trouble figuring out when to make the water molecule and when not to.
calculate the mass of agcl and h2s formed when 85.6 g of ag2s reacts with excess hcl.
Grignard reagents (RMgX) are extremely strong bases and nucleophiles. Comlete the following reactions which demonstrate these two properties.
Plan and Design Lab: To Determine the water of crystallization of a hydrated salt XY•nH2O and to determine the value of n in the formula XY•nH2O with a relative formula mass of 392.14.
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