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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

A reaction mixture contains 0.0500 M NO, 0.0155 M Cl2, and 1.50 M NOCl for the reaction shown below: 2NO(g) + Cl2(g) ⇌ 2NOCl(g)              KC = 46000 at 400 K Show all your work and setup for credit. A) Calculate QC for the reaction. B) Is the reaction at equilibrium? C) If the reaction is not at equilibrium, will it proceed to form more reactants or more product?

Given the following four aqueous solutions (assume complete dissociation): Solution 1 0.30 m CH3OH Solution 2 0.32 m NH3 Solution 3 0.11 m MgSO4 Solution 4 0.18 m KBr   1) Which solution has the highest osmotic pressure? [a] 2) Which solution has the lowest boiling point? [b] 3) Which solution has the highest freezing point? [c] 4) Which solution has the lowest vapor pressure? [d]