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Select the substance with the weakest dispersion force from each of the following pairs. 1) BF3 or BCl3 [a] 2) CH3CH3 or CH3CH2CH2CH3 [b] 3) CCl4 or CF4 [c]

1.00 mol SO3 is placed in a 1.00 L vessel at 425 K and allowed to come to equilibrium at which time 0.500 mol SO3 remains. 2SO3(g) ⇌ 2SO2(g) + O2(g) A) Calculate the equilibrium concentration of SO2(g) [a] mol/L B) Calculate the equilibrium concentration of O2(g) [b] mol/L C) Calculate KC [c] D) Calculate KP [d]

A reaction vessel is charged with COF2, which partially decomposes to carbon dioxide and carbon tetrafluoride. 2COF2(g) ⇌ CO2(g) + CF4(g) When the system comes to equilibrium at 1000oC,  partial pressure of COF2 = 1.50 atm, partial pressure of CO2 = 0.135 atm and partial pressure of CF4 = 0.255 atm. Show all your work and setup for credit. A) Calculate KP for this reaction. B) Calculate KC for this reaction.

Consider the following reaction: N2(g) + O2(g) → 2NO(g) If the initial concentration of N2 was 0.250 M and the concentration of N2 was 0.125 M after 0.100 s, what is the rate of the reaction?

An equilibrium that strongly favors products has ____________

Predict the ideal van’t Hoff factor (i) for Na2SO4

Consider the following reaction: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) If the initial concentration of Cl2 was 0.780 M and the concentration of Cl2 was 0.480 M after 166.0 s, what is the rate of the reaction?

How much heat (in J), is necessary when 54.0 g of ice at

Given the following data, determine the rate law for the following reaction. 2A  + 3B → 2D Experiment [A] [B] Rate (M/s) 1 2.21 1.00 0.619 2 4.42 1.00 1.24 3 3.36 2.40 2.26

A 1.00 L of an aqueous solution contains 1.25 g of a nonionic solute. If the osmotic pressure of this solution at 25 oC is 0.2668 atm. 1) Calculate the molarity of the solution. [A] mol/L 2) Calculate the moles of the nonionic solute in the solution. [B] mol 3) Calcullate the molar mass of the nonionic solute. [C] g/mol