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@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1587 M for H2 and 0.1421 M for I2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HI?H2(g) + I2(g) → 2HI(g) Kc = 48.7000

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.1611 M A, 0.5000 M B, and 0.1611 M C. Which change will cause Qc to be greater than Kc? Use the reaction below.5A → 2 B +3 C Kc = 0.644

@X@user.full_name@X@ @GMU: Determine the rate of consumption of H2 if the rate for formation of NH3 is 0.258 M/s. Use the reaction below.N2(g) + 3 H2(g) → 2NH3(g)

@X@user.full_name@X@ @GMU: Which equation describes the rate of a bimolecular reaction?

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1306 M for N2 and 0.1140 M for O2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of NO?N2(g) + O2(g) → 2NO(g) Kc = 2.70e-18

@X@user.full_name@X@ @GMU: The osmotic pressure of a 14.553 mM solution of (NH4)3PO4 is 732.624 mm Hg at 32.02 °C. How many ions per formula unit of (NH4)3PO4 must there be? The compound may not be completely ionic.

@X@user.full_name@X@ @GMU: What is the mole fraction of potassium chloride, KCl, in an aqueous solution that contains 1.8434 g of potassium chloride dissolved in 24.5581 grams of water? MW(KCl) = 74.551 g/mol.

@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 2.32e-3 M-1/2s-1 at 504.83°C?CH3CHO(g) → CH4(g) + CO(g)

@X@user.full_name@X@ @GMU: What is the activation energy (in kJ/mol) for the reaction below if the rate constants are 2.700e-4 M-1s-1 at 327.00°C and 7.60e-4 M-1s-1 at 346.26°C?H2(g) + I2(g) → 2HI(g)

@X@user.full_name@X@ @GMU: Determine the mole fraction of cyclopentene if 9.4458 g of cyclopentene, C5H8, was mixed with 5.54 g of toluene, C7H8. MW(C5H8) = 68.119 g/mol; MW(C7H8) = 92.141 g/mol.