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@X@user.full_name@X@ @GMU: What is the pH of 6.69e-3 M H2SO4 ?

@X@user.full_name@X@ @GMU: By how much would the rate of reaction (see below) change if the concentration of HCOOH increased by a factor of 1.764. The rate law of this reaction is Rate = k[Br2].HCOOH(aq) + Br2(aq) → 2Br-(aq) + CO2(g)

@X@user.full_name@X@ @GMU: The reaction below is an endothermic reaction. What would one have to do to shift the equilibrium to the right?[Co(H2O)6]Cl2(aq)→[CoCl2(H2O)4](aq) + 2H2O(g)

@X@user.full_name@X@ @GMU: What is the pOH of 1.05e-5 M HBr?

@X@user.full_name@X@ @GMU: NO2 at 378°C decomposes to form NO and O2 according to second order kinetics (see reaction below). The half-life for this reaction was measured to be 2.56e1 s when the initial concentration of NO2 was 9.54e-3 M. What is the rate constant for this reaction?2NO2(g) → 2NO(g) + O2(g)

@X@user.full_name@X@ @GMU: In which substance is the intermolecular bonding best described as hydrogen bonding?

@X@user.full_name@X@ @GMU: What is the concentration of OH- in 0.1106 M CH3COOH ? See reaction belowCH3COOH + H2O → CH3COO- + H3O+ Ka = 1.760×10-5

The two major causes of dead space ventilation are:

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3709 M A, 0.2658 M B, and 0.1997 M C. Which change will cause the equilibrium to shift from left to right if the reaction is exothermic? Use the reaction below.4A(aq) → 3B(aq) +4C(aq) K = 0.600

In patients with closed-head injuries, what may happen in the presence of hypercapnea?