@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)

@X@user.full_name@X@ @GMU: It took 876.9 s for 46.41% 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 value of Kc at 25.00 °C for the reaction below if Kp is 2.5600 at this temperature?2NO(g) + Br2(g) → 2NOBr(g)

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

@X@user.full_name@X@ @GMU: What is the mole fraction of magnesium nitrate, Mg(NO3)2, in an aqueous solution that contains 1.7596 g of magnesium nitrate dissolved in 22.2333 grams of water? MW(Mg(NO3)2) = 148.315 g/mol.

@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.