Blog

A zero-order reaction A → B, has a rate constant of 0.725 M. s-1. How many seconds will it take for the concentration of A to decrease from 2.00 M to 1.25 M?

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 0.3207 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

Select the strongest intermolecular force in each of the following. 1) Br2 – [a] 2) CH4 – [b] 3) NH3 – [c] 4) BF3 – [d] 5) CH3Cl – [e]

The vapor pressure of a liquid is 47.1 kPa at 501 K and 10.5 kPa at 489 K. What is the enthalpy of vaporization of the liquid ? You must show all of your work including units for credit.

Consider the following reaction: 2HI(g) → H2(g) + I2(g) If the initial concentration of HI was 0.350 M and the concentration of HI was 0.025 M after 0.100 s, what is the rate of the reaction?

Octane has a vapor pressure of 40. torr at 318.3 K  and 400. torr at 377.2 K. What is its heat of vaporization? You must show all of your work including units for credit.

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]  

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.