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Select the conjugate acid of the following bases:

Consider the following reaction: N2O4(g) ⇌ 2NO2(g)   Kp = 47.9 at 400 K Suppose that 1.00 atm of N2O4 decomposes and reaches equilibrium at 400 K. Determine the partial pressure of NO2 at equilibrium. Show all of your work including the ICE chart for credit.

Which of the following set of acids and conjugate bases would buffer most effectively at pH = 3.00?

For the reaction 2A + B + C → D + 2F, the rate law is: rate = k[A]2[B][C]-1 Which of the following statements is false?

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

Calculate the pH of a buffer containing 3.50 M formic acid, HCOOH (Ka = 1.8 × 10-4) and 1.25 M sodium formate, HCOONa.You must show all of your work for credit.

1. Select the strongest acid from the following: A) HClO or HClO2 [a] B) HI or HBr [b] 2. Select the strongest base from the following: C) NO2- or NO3- [c] 3. Which will be more soluble in an acidic solution? D) CuCO3 or CuBr2 [d]

Which of the following is true for a chemical reaction at equilibrium?

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