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In a closed 1.00 L flask, 2.60 atm of CO reacts with 5.80 atm of O2 according to the equation below. Assuming that the temperature remains constant, what is the final pressure in the flask?2 CO(g) + O2(g) ? 2 CO2(g)
Assuming that the water is contaminated, devise a method for disposing of the contaminated water without contaminating the environment, but allowing the recycling plant to resume operations as soon as possible.
What mass of sodium chloride, NaCl, is needed to make 389. g of a 3.89%(m/m) NaCl solution? (atomic masses: Na = 22.99, Cl = 35.45)
Explain Gibbs-Duhem Equation, In a certain binary solution, the activity of component 1 is given by
The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. But given the same kinetic energies, a lighter molecule will move faster than a heavier molecule.
when liquid water is put into an evacuated vessel at 25 celsius what is the sign of the change in enthalpy, entropy, free energy, and temperature for the system during this process?
What is the theoretical yield when 0.040 g benzophenone is added to 1 mL methyl alcohol?
Write lewis structures for each of the following species. Use expanded octects as necessary.
A mixture of Helium, Neon, and Nitrogen gases has a pressure of 1.348 atm. Determine what is the partial pressure of N2 in the mixture If the pressures of Helium and Neon are 0.124 atm and 0.996 atm, respectively.
What is the rate of the above reaction? What is the closest numerical value of K for the above reaction? What are the units for the rate constant for the reaction?
when a .28 gram sample of limestone was decomposed by heating 75 millileters of CO2 at 750 mm Hg and 20 degrees celcius were evolved. How many grams of CO2 were produced?
Calculate the wavelength in nanometers of the spectral line in the visible spectrum of hydrogen for which n1 = 2 and n2 = 3. What color is this line?
What mass of sucrose should be combined with 464 g of water to make a solution with an osmotic pressure of 8.35 atm at 320 K? (Assume the density of the solution to be equal to the density of the solvent.)
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