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@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1506 M for H2 and 0.1223 M for Br2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HBr?H2(g) + Br2(g) → 2HBr(g) Kc = 1.42e3

Which of the following conditions will cause equilibrium to shift to the left?2NH3(g) + ⇋ N2(g) + 3H2(g)

@X@user.full_name@X@ @GMU: Determine the rate of consumption of I− if the rate for formation of I2 is 0.333 M/s. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

@X@user.full_name@X@ @GMU: The following data was obtained by the method of initial rates. What is the rate law for the reaction of A with B to produce product? [A]o [B]o Rate, M/s 0.289 0.300 2.10e-7 0.483 0.300 4.54e-7 0.289 0.552 3.87e-7

@X@user.full_name@X@ @GMU: Determine the rate of formation of I3− if the rate for formation of SO42− is 0.400 M/s. Use the reaction below.3I−(aq)+ S2O82−(aq) → I3−(aq) + 2SO42−(aq)

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.3075 M A, 0.2127 M B, and 0.1435 M C. Which change will cause the equilibrium to shift from right to left if the reaction is exothermic? Use the reaction below.2A(aq) → 3 B(aq) +3 C(aq) K = 0.406

@X@user.full_name@X@ @GMU: What is the activation energy (in kJ/mol) for the reaction below if the rate constants are 1.050e-3 M-1/2s-1 at 486.00°C and 2.82e-3 M-1/2s-1 at 509.55°C?CH3CHO(g) → CH4(g) + CO(g)

What would be the expected rate law for the mechanism described below?1 Cl + O3 → ClO + O2 slow 2 ClO + O → Cl + O2 fast

@X@user.full_name@X@ @GMU: The osmotic pressure of a 18.402 mM solution of NaOH is 445.257 mm Hg at 26.58 °C. How many ions per formula unit of NaOH must there be? The compound may not be completely ionic.

@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?