@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)

@X@user.full_name@X@ @GMU: A mixture containing an initial concentration of 0.1942 M for H2 and 0.1665 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

@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)

@X@user.full_name@X@ @GMU: What is the activation energy (in kJ/mol) for the reaction below if the rate constants are 1.080e9 M-1s-1 at -78.00°C and 2.06e9 M-1s-1 at -59.21°C?NO(g) + O3(g) → NO2(g) + O2(g)

@X@user.full_name@X@ @GMU: Radioactive substances decay by first-order kinetics. How many years would be required for a sample containing carbon-14 to decrease to 53.91% of its initial activity? The half-life of carbon-14 is 5.73e3 years.

@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: It took 991.5 s for 55.53% of a substance to react according to first-order kinetics. What is the value of the rate constant?

@X@user.full_name@X@ @GMU: What is the overall order of the elementary reaction:3*A + 2*B → C?

@X@user.full_name@X@ @GMU: Determine the rate of formation of I3− if the rate for consumption of I− is 0.249 M/s. Use the reaction below.3I−(aq)+ S2O82−(aq) → I3−(aq) + 2SO42−(aq)

@X@user.full_name@X@ @GMU: How many grams of potassium hydroxide, KOH, would be required to prepare a 0.2434 m KOH solution by combining this compound with 0.3947 L of water (assume a density of 1.00 g/mL)? The molecular weight is 56.1056 g/mol.