General Chemistry 2

Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

$$NO_2 + CO~ \xrightarrow{k_1}~ NO + NO_3$$ $$NO_3 + CO~ \xrightarrow{k_2}~ NO_2 + CO_2$$
Find equilbirium concentrations of each species when starting with 3.0 M I\(_2\)

I\(_2\) (g) \(\leftrightharpoons\) 2 I (g) , K\(_C\) = 3.8 x 10\(^{-5}\)
In the below reactions, identify which reactant is the lewis acid and which is the lewis base.

NH\(_3\) + BF\(_3\) \(\leftrightharpoons\) NH\(_3\)BF\(_3\)

KOH + CH\(_3\)Br \(\leftrightharpoons\) KBr + CH\(_3\)OH
Calculate the pH and concentration of all species of a 3.0 M solution of phosphoric acid, H\(_3\)PO\(_4\)
What is the molar solubility of Ag\(_2\)CrO\(_4\) in 0.100 M AgNO\(_3\)? Compare this to the molar solubility of Ag\(_2\)CrO\(_4\) in water, 1.3 x 10\(^{-4}\) M

Ag\(_2\)CrO\(_4\) K\(_{sp}\) = 9.0 x 10\(^{-12}\)
Assign oxidation numbers for the species below. Determine which species is the oxidizing agent and which is the reducing agent. Which species is being oxidized? Which species is being reduced?

Cr\(^{3+}\) + Pb \(\longrightarrow\) Cr + Pb\(^{2+}\)
Below is a proposed mechanism for a reaction, with k1 > k2. What is the rate law?

$$NO+ Br_2~ \mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~ NOBr_2$$ $$NOBr_2 + NO~ \xrightarrow{k_2}~ NOBr + NOBr$$
A 3.050 L reaction vessel contains 0.3500 mol CO, 0 mol Cl\(_2\), 0.05500 mol COCl\(_2\). Find the molarity of Cl\(_2\) at equilibrium.

CO + Cl\(_2\) \(\leftrightharpoons\) COCl\(_2\) , K\(_C\) = 1200
Hydrogen bromide is a gas at room temperature. It is soluble in water, forming hydrobromic acid. Identify the conjugate acid-base pairs.
HBr (aq) + H\(_2\)O (l) \(\longrightarrow\)
What is the pH of a 0.1 M sulfuric acid solution? (did you know sulphuric is an alternative spelling?)

H\(_2\)SO\(_4\) + H\(_2\)O \(\longrightarrow\) HSO\(_4^-\) + H\(_3\)O\(^+\), K\(_{a1}\) = 1.0 x 10\(^{3}\)

HSO\(_4^-\) + H\(_2\)O \(\longrightarrow\) SO\(_4^{2-}\) + H\(_3\)O\(^+\), K\(_{a2}\) = 1.2 x 10\(^{-2}\)

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