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Calculate ΔSsurr at 298 K. 2NO(g) +  O2(g) → 2NO2(g) ΔH = -114 kJ

Predict the ideal van’t Hoff factor (i) for K3PO4.

Calculate the mass of iron metal that will be deposited by passing a 85.0 A current through a solution of iron(II) chloride for 15.0 minutes. Fe2+(aq) + 2 e⁻  →  Fe(s)  You must show all of your work including units for credit.

Predict the ideal van’t Hoff factor (i) for KNO4.

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.