# General Chemistry 2

The initial concentration of hydroiodic acid is 100 mmol/L but after 500 s it is 17 mmol/L. What is the rate? (note the products of this reaction are hydrogen and iodine gas)

The following initial rate data was collected for the reaction, A + 2B $\longrightarrow$ products

B. Find the rate constant

When cyclopropane is heated to 500 $^\circ$C it changes to propene. The following data was obtained from experiment:

Confirm that the reaction is 1st order and calculate the rate constant.

An isotope of phosphorous, $^{32}$P, is radioactive and undergoes beta decay with a half life of 14.3 days. How long would it take for 99% of a sample of this isotope to decay?

For a given reaction, the reaction rate exactly doubles when the temperature is raised from 293 K to 304 K. Calculate the activation energy.

For the mechanism proposed below, determine the overall rate law for k$_1$ < k$_2$, k$_1$ > k$_2$

$2~NO~+~2 H_2~\longrightarrow~2~H_2O~+~N_2~~{overall}$

$2~NO+~H_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~N_2O~+~H_2O$

$N_2O~+~H_2~\xrightarrow{k_2}~N_2~+~H_2O$

For the mechanism below, determine the overall rate law.

$2~NO~+~Br_2~\longrightarrow~2~NOBr~~{overall}$

$NO+~Br_2~\mathop{\leftrightharpoons}^{k_1}_{k_{-1}}~NOBr_2$

$NOBr_2~+~NO~\xrightarrow{k_2}~2NOBr$

Find the rate law for the following reaction mechanism using the pseudo(quasi) steady state hypothesis

$A + B~\longrightarrow~C$

$C~\longrightarrow~D$

Find the equilibirium concentrations when starting with 0.50 M H$_2$ and 0.50 M Br$_2$

H$_2$ + Br$_2$ $\leftrightharpoons$ 2 HBr , K$_C$ = 143

A 2.16 L reaction vessel contains 0.186 mol HCONH$_2$, and 0 mol of NH$_3$ and CO. How many moles of each substance are in the equilibrium mixture at 400 K? What is the pressure in the vessel?

HCONH$_2$ $\leftrightharpoons$ NH$_3$ + CO , K$_C$ = 4.84

Lactic acid, HC$_3$H$_5$O$_3$, is a waste product that accumulates in muscle during exertion, leading to pain and a feeling of fatigue. In a 0.100 M aqueous solution, lactic acid is 3.7% dissociated. Calculate the value of K$_a$ for this reaction.

Compare the concentration of H$_3$O$^+$ in 1 M and 2 M solutions of HC$_2$H$_3$O$_2$, K$_a$ = 1.8 x 10$^{-5}$. (doubling the concentration results in an increase of hydronium ions by what factor?)

Calculate the pH of a mixture of equal parts 2.0 M HF and 1.0 M HOCl. Also find the concentration of OCl$^-$ and F$^-$ ions in the solution. The K$_a$ of HF = 7.2 x 10$^{-4}$, K$_a$ of HOCl = 3.5 x 10$^{-8}$

Calculate the pH of 0.1 M NH$_4$Cl. The K$_b$ of NH$_3$ = 1.8 x 10$^{-5}$

Calculate the pH of 0.12 M KNO$_2$. The K$_a$ of HNO$_2$ = 4.0 x 10$^{-4}$

Find the pH of a 0.1 M solution of NH$_3$. If 50 ml of this solution is titrated by 50 ml of 0.1 M HCl, find the pH at the equivalence point. (K$_a$ = 5.56 x 10$^{-10}$ )

Calculate the solubility (in grams per liter) of PbI$_2$ in water from the solubility product constant 1.4 x 10$^{-8}$.

Calculate the equilibrium concentration of Pb$^{2+}$, I$^-$, Na(\^+$, and NO$_3^-$when 100.0 mL of 0.0500 M Pb(NO$_3$)$_2## and 200.0 mL of 0.100 M NaI are mixed.

PbI$_2$ K$_{sp}$ = 1.4 x 10$^{-8}$

The concentration of Mg(NO$_3$)$_2$ is 4 x 10$^{-4}$ M and the concentration of NaOH is 2 x 10$^{-4}$, do you expect Mg(OH)$_2$ to precipitate?

Mg(OH)$_2$ K$_{sp}$ = 8.9 x 10$^{-12}$

What is the solubility of AgCl in 0.020 M NaCN?

AgCl K$_{sp}$ = 1.8 x 10$^{-10}$

Ag(CN)$_2^-$ K$_{f}$ = 5.6 x 10$^{18}$