@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 7.67e-4 M-1s-1 at 346.45°C?H2(g) + I2(g) → 2HI(g)

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

@X@user.full_name@X@ @GMU: What is the value of Kc at 226.85 °C for the reaction below if Kp is 6.24e-3 at this temperature?CO(g) + 2H2(g) → CH3OH(g)

What would be the expected rate law for the mechanism described below?1 O3(g) + HO(g) → HO2(g) + O2(g) fast 2 HO2(g) + O → OH(g) + O2(g) slow

@X@user.full_name@X@ @GMU: Initially there were equilibrium concentrations of 0.1696 M A, 0.2500 M B, and 0.1696 M C. Which change will cause the equilibrium to shift from right to left? Use the reaction below.3A → 4 B +2 C Kc = 0.784

@X@user.full_name@X@ @GMU: Determine the rate of consumption of I− if the rate for formation of I2 is 0.261 M/s. Use the reaction below.IO3− + 5I− + 6H+ → 3I2 + 3H2O

Sulfuryl Chloride, SO2Cl2 decomposes in the gas phase according to first order kinetics. Determine half-life and the rate constant.SO2Cl2(g) → SO2(g) + Cl2(g)

@X@user.full_name@X@ @GMU: What is the solubility in g/L of Kr at a partial pressure of 268.1 torr, if the solubility at a partial pressure of 431.8 torr is 0.1328 g/L?

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1408 M for H2 and 0.1161 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 a exothermic reaction. What would one have to do to shift the equilibrium to the right?4NO(g) + 6H2O(g)→4NH3(g) + 5O2(g)