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White phosphorus is a molecular solid made of molecules of P4. A 3.88 g sample of white phosphorus starts at 24oC. Calculate the amount of heat (in J) required to melt the sample. Use the following data: Tp = 44oC; C = 94 JoC-1 mol-1; ΔHfusion = 2.5 kJ/mol.
Calculate [H+] and the pH of the following solutions
how many liters of 13.5 molar HCl stock solution are needed to make 10.5 liters of a 1.8 molar HCl solution?
calculate the approximate concentration of the solution in mol/kg and determine the volume change of the ballon when it ascends from 1 atm pressure to 240 torr pressure ?
At a given temperature, the equilibrium constant K for the reaction 2SO2(g) + O2(g) 2SO3(g) is 3.0 × 109. If 2.80 mol of SO2 and 4.06 mol of O2 are placed in a 1.78-L container.
Application of ideal gas law - How high can you raise the temperature of the gas without bursting the vessel?
When 9.00 grams of Al react with an excess of H3PO4, 30.0 grams of ALPO4 are produced.What is the percentage yeild of this reaction.
What is the solubility product constant? Given Ksp = 1.1 x 10^-3 for BaF2(s), calculate the molarity of Ba+2 in a saturate solution of BaF2 (at equilibrium).
Calculate the molar mass of the unknown gas. (remember that the faster the rate of effusion, the shorter the time required for effusion of 1.0L
Calculate the mass of oxygen dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air
Determine the V of a voltaic cell (E°cell) if it is required to do 5.43 × 10¯3 Kilo Joule of work when a charge of 2.50 C is transmitted.
Calculate the percent by weight, mole fraction and mole percent of each component in a mixture consisting 9g of water (H2O), 120g acetic acid(CH3COOH) and 115g of ethyl alcohol (C2H5OH).
A 29.0-g sample of water at 260. K is mixed with 51.0 g water at 340. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
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