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@X@user.full_name@X@ @GMU: What would the [OH-] be after addition of 15.04 mL of 0.1000 M NaOH to 25.00 mL of 0.1000 HA (a weak acid, Ka = 5.86e-5)?

@X@user.full_name@X@ @GMU: Which base listed below would be the best to creat a buffer having a pH of 9.3373?

@X@user.full_name@X@ @GMU: Determine the concentration of A after 91.005 seconds if the initial concentration of A was 0.3741 M and the first order rate constant is 1.265e-2 s-1.

@X@user.full_name@X@ @GMU: What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 2.08e-7?4C2H2(g) + 5 H2(g) → C8H18(g) ΔGo = -819.870 kJ.

@X@user.full_name@X@ @GMU: If you raise the pressure from what it is at point 1 to that of point 5, you go from a ___ to _____.

@X@user.full_name@X@ @GMU: Which of the answers below is the correct representation according to the shorthand method of the following galvanic cell?Ni2+(aq) + Al(s) → Ni(s) + Al3+(aq)

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of H+ increased by a factor of 1.525. The rate law of this reaction is Rate = k[BrO3-][Br-][H+]2.BrO3- + 5Br- + 6H+ → 3Br2 + 3H2O

@X@user.full_name@X@ @GMU: To what temperature would you have to heat Ni(l) to cause its vapor pressure to become 186.4 mm Hg if its heat of vaporization and boiling point are 428.00 kJ/mol and 3005.2 K, respectively?

@X@user.full_name@X@ @GMU: The osmotic pressure of an unknown solution is 403.809 mm Hg at 17.78 °C. Which of the solutions below is the most likely one? Assume any salt is completely ionic!

@X@user.full_name@X@ @GMU: What is the rate constant at 503.62°C for the reaction below if the rate constant is 1.05e-3 M-1/2s-1 at 486.00°C and the activation energy is 207.00 kJ/mol?CH3CHO(g) → CH4(g) + CO(g)