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@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1074 M for H2 and 0.0808 M for Cl2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HCl?H2(g) + Cl2(g) → 2HCl(g) Kc = 5.00e16

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1738 M for H2 and 0.1430 M for Cl2 is allowed to come to equilibrium (see reaction below). What must be the equilibrium concentration of HCl?H2(g) + Cl2(g) → 2HCl(g) Kc = 5.00e16

@X@user.full_name@X@ @GMU: The reaction below is an endothermic reaction. What would one have to do to increase the size of the equilibrium constant?SO2Cl2(g)→SO2(g) + Cl2(g)

Determine if the reverse reaction for the energy level diagram is endothermic or exothermic and what the ΔH for the forward reaction is.

@X@user.full_name@X@ @GMU: Determine the mole fraction of toluene if 7.1397 g of toluene, C7H8, was mixed with 6.86 g of benzene, C6H6. MW(C7H8) = 92.141 g/mol; MW(C6H6) = 78.114 g/mol.

@X@user.full_name@X@ @GMU: The reaction below is an endothermic reaction. What would one have to do to increase the size of the equilibrium constant?CaCO3(s)→CaO(s) + CO2(g)

@X@user.full_name@X@ @GMU: Radioactive substances decay by first-order kinetics. How many days would be required for a sample containing phosphorus-32 to decrease to 67.66% of its initial activity? The half-life of phosphorus-32 is 1.42e1 days.

@X@user.full_name@X@ @GMU: What is the solubility in mol/L of H2S at a partial pressure of 374.5 torr, if the solubility at a partial pressure of 507.7 torr is 0.06614 mol/L?

@X@user.full_name@X@ @GMU: Determine the mole fraction of cyclohexene if 5.4922 g of cyclohexene, C6H10, was mixed with 6.00 g of cyclopentene, C5H8. MW(C6H10) = 82.145 g/mol; MW(C5H8) = 68.119 g/mol.

@X@user.full_name@X@ @GMU: Determine the mass of LiI required to produce a 0.2990 molal solution by dissolving LiI in 126.7747 g of H2O.