Given the following data, determine the rate law for the following reaction. 2A + B + 2C → products Experiment [A] [B] [C] Rate (M/s) 1 0.273 0.763 0.400 3.0 2 0.819 0.763 0.400 9.0 3 0.273 1.526 0.400 12.0 4 0.273 0.763 0.800 6.0

Select the substance with the stronger dispersion force from each of the following pairs. 1) Cl2 or Br2 [a] 2) CO2 or CS2 [b] 3) SiCl4 or CF4 [c]

What is the boiling point of a solution prepared by dissolving 320.0 g of S8 (molar mass = 256.5 g/mol) in 1500.0 g of CCl4? (Kb = 5.05oC/m, boiling point of pure CCl4 = 76.7oC)

Consider the following 1.0 M aqueous solutions: A) HClO(aq) B) NaOH(aq) C) HNO3(aq) D) NH3(aq) Rank the aqueous solutions from the highest pH to the lowest pH. highest pH —–> [1] [2] [3] lowest pH —–> [4]  

For the reaction , N2(g) + 3H2(g) → 2NH3(g), the rate of formation of NH3 is 0.345 M/s. What is the corresponding rate of disappearance of N2 ?

Consider the following equilibrium: CO(g) + H2O(g) ⇌ H2(g) + CO2(g)   Kc = 16 Suppose that 1.50 mol of CO  and 1.50 mol of H2O are placed in 0.500 L flask and allowed to come to equilibrium at high temperature. A) Calculate the equilibrium concentration of CO2(g) [a] mol/L B) Calculate the equilibrium concentration of H2O (g) [b] mol/L C) Calculate the equilibrium concentration of H2(g) [c] mol/L D) Calculate the equilibrium concentration of CO (g) [d] mol/L

Consider the following equilibrium: CO(g) + H2O(g) ⇌ H2(g) + CO2(g)   Kc = 16 Suppose that 1.00 mol of CO  and 1.00 mol of H2O are placed in 0.500 L flask and allowed to come to equilibrium at high temperature. A) Calculate the equilibrium concentration of CO2(g) [a] mol/L B) Calculate the equilibrium concentration of H2O (g) [b] mol/L C) Calculate the equilibrium concentration of H2(g) [c] mol/L D) Calculate the equilibrium concentration of CO (g) [d] mol/L

For the reaction , N2(g) + 3H2(g) → 2NH3(g), the rate of formation of NH3 is 0.345 M/s. What is the corresponding rate of disappearance of H2 ?

For the reaction 2A + 3B → 4C + 5D, how does the rate of disappearance of B compare to the rate of production of C?

The half-life of a first-order reaction is 0.300 s. What is the rate constant?