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One mole of an ideal monoatomic gas initially at 300 K is expanded from an initial pressure of 10 atm to a final pressure of 1 atm. The molar heat capacity for constant volume for the gas is 32VCR=. Calculate dU, dH, q, w, and the final temperature (Tf) for each of the following paths:
(a) An expansion against a constant external pressure of 1 atm in a thermally isolated (adiabatic) system.
(b) An expansion against zero external pressure (against a vacuum) in an adiabatic system.
balanced equation for the preparation of the diazonium ion that i have made. draw possible structure for the azo dye.
calculating the equilibrium constant keq for the given reactions.calculate the keq for the following reactions.n2gnbsp
If one started will 6.73 g of copper chloride, how many grams of copper could be produced?
The observations listed were made on different solns. Given the observations state which ion studied in this experiment is present. If the test is not definitive, indicate that with a (?).
carbon dioxide is a green house gas that is linked to global warming. it is released into the atmosphere through the
A compound is known to have a free amino group with a pKa of 8.8, and one other ionizable group with a pKa between 5 and 7. To 100 mL of a 0.2 M solution of this compound at pH 8.2 was added 40 mL of a solution of 0.2 M hydrochloric acid.
Determine whether each of these species follows the octet rule, is octet deficient (central atom works with less than eight electrons in its valence shell), or has an expanded octet (central atom works with more than eight electrons in its valence..
An aqueous solution that contains 285ppm of potassium nitrate (KNO3) is being used to feed plants in a garden. What volume of this solution is needed.
Mg3N2 + 6H2O ----> 3Mg(OH)2 + 2NH3 When 36.0g of H2O react, how many grams of NH3 are produced?
A Vessel of of volume 22.4 L contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.
determine the number of carbon atoms in the compound. Natural abundances: 12C is 98.93% and 13C is 1.07%
Assume you have a solution containing two volatile liquids. Given the data for liquid A: MM = 56.89 g/mole, partial pressure = 0.903 atm and for liquid B: MM = 14.52 g/mole, partial pressure = 0.995 atm
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