Throwback Thursday Quiz #4

• Because two molecules of NO are consumed per molecule of O₂, the rate of disappearance of O₂(g) is 2.5 x 10^-5 Ms^-1.

• Because two molecules of NO are consumed per molecule of O₂, the rate of disappearance of O₂(g) is 1.0 x 10^-4 Ms^-1.

• Because the rate depends on [NO]² and [O₂], the rate of disappearance of O₂(g) is 2.5 x 10^-9 Ms^-1.

• Because the O₂(g) is under the same experimental conditions as NO, it is consumed at the same rate of 5.0 x 10^-5 Ms^-1.

• The rate of reaction will remain the same, because k will decrease by half.

• The rate of reaction will double, because the rate is directly proportional to [S₂O₈^2-].

• The rate of reaction will increase by a factor of four, because two moles of SO₄^2- are produced for each mole of S₂O₈^2- consumed.

• The rate of reaction will increase by a factor of four, because the reaction is second order overall.

• Rate = k

• Rate = k[HO₂]

• Rate = k[HO₂]²

• Rate = k[H₂O₂][O₂]

• P₁/9

• P₁/3

• P₁

• 3P₁

Equal volumes of 0.2 M solutions of lead(II) nitrate and potassium bromide are combined to form lead(II) bromide as a yellow precipitate. Which of the following is the correct net ionic equation for the reaction?

To gravimetrically analyze the silver content of a piece of jewelry made from an alloy of Ag and Cu, a student dissolves a small preweighed sample in HNO₃(aq). Ag⁺(aq) and Cu²⁺(aq) ions form in the solution. Which of the following should be the next step in the analytical process?

• Centrifuging the solution to isolate the heavier ions

• Evaporating the solution to recover the dissolved nitrates

• Adding enough base solution to bring the pH up to 7.0

• Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions