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The vapor pressure of br2(l) at 25C is 228 mm hg. if 2.00g of br2 is usedm what is the final pressure in the flask? will there be liquid in the flask?
Determine How hot should be the air in a ballon be heated if it has initially a volume of 750. L at the temperature of 20 degree celsius and the final volume must be 1,000.l
Find the mass of the substance and the volume of a gas in a reaction - determine the mass of solid ammonium nitrate that must be used to obtain 0.145 L of dinitrogen oxide gas at STP.
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?
The evaporation of water H2O(l) ->H2O(g) is endothermic: Change in T degree +44.01 kJ Determine the minimum mass of water (in ) has to evaporate to absorb 183 joules of heat?
Specific rotation of α and β -D-glucose - Determine the percentage of each anomer at equilibrium.
Determine the mole fraction of sodium chloride(NaCl) in the solution if this solution is formed by mixing 17.0 grams of sodium chloride NaCl in 85.0 grams of Water?
it is observed that a volume of 29.15 mL of KOH was neede to complete the process of titration. Determine what is the concentration of this unknown HCl solution?
Determine the freezing point and calculate the final temperature if initially this iron nail was at temperature of 28 degree Celsius?
Determine What is the ? Ssys for the process?(if it is given the specific heat capacity for ethanol is 2.42 J/g K.) express your answer in units of J/K
Determine the pressure (in atm) inside the can if a metal can of 1.00 qt contains 0.150 grams of Helium at a temperature of 20 degrees Celsius also explain Is this pressure greater or less than standard atmospheric pressure?
the ratio of the no of molecules in the excited state at the temperature of 213 K to the number of ground state molecules and the percent of the excited molecules at 213 K.?
Determine the partial pressure and the total pressure using Dalton's law of partial pressures - Determine the total pressure of the mixture.
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