General Chemistry 2

Consider a solution of 0.10 M H$^{+}$ in 0.10 M thioacetimide at 25 $^\circ$C

rate = k[H$^{+}$][CH$_3$CSNH$_2$]

How are the rate and the rate constant (k) effected when water is added to the solution? When the reaction is heated to 75$^\circ$C ? When NaOH is added?

Derive the rate law given the elementary steps.

$Cl_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~2~Cl~~{1}$

$Cl+~CHCl_3~\xrightarrow{k_2}~HCl~+~CCl_3~~{2}$

$Cl~+~CCl_3~\xrightarrow{k_3}~CCl_4~~{3}$

For the proposed mechanism below, identify the intermediates and determine the rate law.

$2~NO_2~+~F_2~\leftrightharpoons~2~NO_2F~~{overall}$

$NO_2F_2+~Br_2~\longrightarrow~NO_2F~+~F~~{slow step}$

$NO_2~+~F~\longrightarrow~NO_2F$

For the proposed mechanism below, find the overall reaction, identify the intermediates, then determine the rate law.

$CL_2~\leftrightharpoons~2~Cl$

$2~Cl~+2~NO~\longrightarrow~2~NOCl$

A 1.9 L vessel contains a gaseous mixture with 0.455 mol SO$_2$, 0.183 mol O$_2$, and 0.568 mol SO$_3$. Is the reaction at equilibrium? If not, what is the direction of the reaction?

2 SO$_2$ + O$_2$ $\leftrightharpoons$ 2 SO$_3$, K$_C$ = 280

A 1 L reaction vessel contains 2.5 mol A, 3 mol B, and initially 0 C. Find the concentrations of all species at equilibrium.

A + 2B $\leftrightharpoons$ 3 C , K$_C$ = 0.25

0.20 M I$_2$ is placed in a reaction vessel. Find the concentrations of I$_2$ and I at equilibrium.

I$_2$ (g) $\leftrightharpoons$ 2 I (g) , K$_C$ = 3.8 x 10$^{-5}$

Starting with 0.50 M N$_2$O$_4$, calculate the equilbrium concentrations of all species involved in the reaction below.

N$_2$O$_4$ $\leftrightharpoons$ 2 NO$_2$ K$_C$ = 1.2

A 2.5 L reaction vessel contains 0.55 mol PCl$_5$, 0.55 mol PCl$_3$, and 0 mol Cl$_2$. Find the molarity of Cl$_2$ at equilibrium.

PCl$_5$ $\leftrightharpoons$ PCl$_3$ + Cl$_2$ , K$_C$ = 3.8 x 10$^{-2}$

0.800 moles of N$_2$ (g) are placed in a 7.00 L flask with 3.00 moles of H$_2$ and allowed to react for some time. After several hours the concentrations of H$_2$ (g) is measured at 0.278 M. What is the equilibrium constant for the reaction at this temperature?

N$_2$ (g) + 3 H$_2$ (g) $\leftrightharpoons$ 2 NH$_3$ (g)

Predict the effect an increase in H$_2$ would have on the following reaction. What if we increase the temperature? If we remove H$_2$O?

CO (g) + H$_2$O (g) $\leftrightharpoons$ CO$_2$ (g) + H$_2$ (g) + heat, K$_C$ = 5.10

What are the factors that affect the strength of an acid?

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

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) $\longrightarrow$

Ammonia is a pungent gas at room temperature. Its main use is in the production of fertilizers and explosives. It is very soluble in water. It forms a basic solution that is used in common products, such as glass cleans. Identify the conjugate acid-base pairs in the reaction between aqueous ammonia and water.

NH$_3$ (aq) + H$_2$O (l) $\longrightarrow$

Predict the products for the following reaction

KHSO$_3$ + NH$_3$ $\leftrightharpoons$ ?

KHSO$_3$ has K$a$ = 6.2 x 10$^{-8}$ K$b$ = 1.0 x 10$^{-4}$

NH$_3$ has K$a$ = 7.8 x 10$^{-13}$ K$b$ = 1.8 x 10$^{-5}$

Find the pH of 2.0 M HF, ( K$_a$ = 7.1 x 10$^{-4}$ )

Find the pH of 3.0 M NH$_3$, ( K$_b$ = 1.8 x 10$^{-5}$ )

Find the pH of a 0.100 M solution of HOCl, K$_a$ = 3.5 x 10$^{-8}$

A solution contains 0.5 M KOH and 0.75 M Cs(OH)$_2$, calculate the pOH of the solution