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The formation enthalpy of NO2 is ?Hf =37.2 kJ/mol. How much heat is required to convert 83 g of nitrogen gas to NO2 at constant temperature and pressure in the presence of excess oxygen
To what final volume should you dilute 60.0mL of a 5.40M KI solution so that 40.0mL of the diluted solution contains 3.75g of KI
How many grams of dry NH_4Cl need to be added to 2.10 L of a 0.100 it M solution of ammonia, NH_3, to prepare a buffer solution that has a pH of 8.84? K_b for ammonia is 1.8 * 10^{-5}
assuming that the gas behaes ideally. Then repeat the calculation by using the van der Waals equation
Is PH3 polar or nonpolar, and why? Some sources say it's polar because of the lone pair. Others say it's nonpolar
Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Using the original buffer solution,
The pKb values for the dibasic base B are pKb1 = 2.1 and pKb2 = 7.8. Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.75 M B(aq) with 0.75 M HCl(aq).
if the height of the mercury column in a leveling bulb is 30 mm greater than that in the gas buret and atmospheric pressure is 670 mm, what is the pressure on the gas trapped in the buret.
Calculate the mass ( kg ) of the solute C4H8O and the volume ( mL ) of the solvent C6H6 that should be combined to generate 6450 g of a solution that is 2.07 m C4H8O.
for a certain change the value of U is -2.37 kJ. During the change, the system absorbs 650 joules. how much work did the system do.
At a certain temperature, Kp = 1.42 for the reaction PCl5 PCl3 + Cl2. Calculate the equilibrium partial pressures and the total pressure if the initial partial pressures are PpCl5= 2.88 atm , PpCl3 = 1.98 atm , and PCl2 = 1.42 atm.
how many grams of chlorine are required to react completely with 5.00grams of sodium to produce sodium chlorde ?
Calculate the equilibrium pressure of the H2O vapour at both 0oC and 25 oC. The value of ?H is 522.0kj/mol, why may be assumed constant over the temperature range of interest.
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