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@X@user.full_name@X@ @GMU: It took 1016.0 s for 40.74% of a substance to react according to first-order kinetics. What is the value of the rate constant?

Consider the reaction.4NH3(g) + 5O2(g) ⇋4NO(g) + 6H2O(l)What is the correct expression for Kc?

@X@user.full_name@X@ @GMU: When 12.26 g of citric acid was dissolved in 108.4 g of benzene, the freezing point was 275.6 K. What is the formula mass of this compound? The freezing point depression constant for benzene is 5.12 (°C*kg)/mol. The melting point and boiling points are 5.50°C and 80.10°C, respectively.

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3038 M A, 0.2819 M B, and 0.1761 M C. Which change will cause the equilibrium to shift from left to right if the reaction is endothermic? Use the reaction below.2A(aq) → 3 B(aq) +2 C(aq) K = 0.543

@X@user.full_name@X@ @GMU: Determine the rate of the last set of reaction conditions. [A]o [B]o Rate, M/s 0.281 0.289 3.71e-5 0.433 0.289 7.08e-5 0.281 0.531 5.03e-5 0.433 0.444 ?

What would be the expected rate law for the mechanism described below?1 NO(g) + 1/2O2(g) → NO2(g) slow 2 NO2(g) → NO(g) + O(g) fast 3 O2(g) + O(g) → O3((g) fast

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.1006 M A, 0.3333 M B, and 0.1006 M C (see reaction below). The concentration of C was suddenly increased to 11.43 M. What was the approximate concentration of each after equilibrium had been re-established?4A → 3 B +4 C Kc = 1.248

@X@user.full_name@X@ @GMU: The reaction below is a exothermic reaction. What would one have to do to shift the equilibrium to the right?2NO2(g)→N2O4(g)

@X@user.full_name@X@ @GMU: It took 286.6 s for 35.22% of a substance to react according to first-order kinetics. What is the value of the rate constant?

What would be the expected rate law for the mechanism described below?1 CH3CH2Br + AlBr3 → AlBr4- + CH3CH2+ slow 2 CH3CH2+ + C6H6 → C6H6CH2CH3+ fast 3 C6H6CH2CH3+ + AlBr4- → AlBr3 + HBr + C6H6CH2CH3 fast